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April 16, 2014

Search: Calculate the pH after naoh is added

Number of results: 64,336

College Chemistry
You weigh a sample of a monoprotic unknown acid and dissolve it in 50.00 mL of distilled water. Exactly half of this solution is titrated with Sodium Hydroxide to the phenolphthalein end point. The pH of the other half of the original solution is measured with a pH meter. The...
Tuesday, April 9, 2013 at 4:31pm by Kim

chemistry
You have 5 points on the titration curve. You must recognize where you are on the curve. At zero mL, you have pure Ba(OH)2 so the pH will be determined by that concn. At the other points, calculate how moles Ba(OH)2 you have initially, the moles HCl added. Calculate moles Ba(...
Monday, March 28, 2011 at 1:19pm by DrBob222

chemistry
What is the pH of the solution created by combining 2.80 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? mL of NaOH pH w/HCl pH w/HC2H3O2 2.80 ? ? okay, so i tried m1v1=m2v2 and when i got m2 i would input it in -log(H+) to...
Wednesday, July 9, 2008 at 12:19am by UN

chemisty
what is the final pH after 1 drop(.05ml) of 6M HCl is added to 1.0L of freshly prepared pure water that was originally at a pH of 7.0. Is there a signigicant pH change?
Monday, March 1, 2010 at 6:30pm by tiffany

Chemistry
You need to do ICE charts for both of these. If we call aspirin, HA, it makes it easier to write. millimoles HA = 20 x 0.07222 = 1.44 mmoles NaOH = 10 x 0.2 = 2.0 ...........HA + NaOH ==> NaA + H2O initial...1.44.................. add.............2.0............ change...-1...
Saturday, November 26, 2011 at 8:14pm by DrBob222

chemistry
A student titrated 10.00mL aliquots of her unknown amino acid solution with standard 0.1521M NaOH and with 0.0986M HCl. Inflection points were determined in the graphs after 3.29mL of HCl and 18.61mL of NaOH were added. Calculate the concentration of the amino acid
Thursday, August 5, 2010 at 2:55am by Brandon

Chem Webwork help
1. What is the pH when enough 0.10 M Base (in mL) is added to neutralize 8 mL of 0.10 M Acid? Complete the following table. NaOH HC2H3O2 2. What is the pH of the solution created by combining 2.60 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of ...
Monday, July 12, 2010 at 2:34am by Sammy

chemistry
what is the pH of a solution containing 25 ml of 0.10M acetic acid after 10 ml of 0.10M NaOH is added?
Sunday, August 8, 2010 at 7:05am by thimmaiah

Chemistry - pH
Calculate the pH of each of the following solutions: a) .35 M hydrochloric acid, HCl b) .35 M acetic acid, HC2H3O2 c) .35 M sodium hydroxide, NaOH Can someone please explain to me how to calculate the pH in a way that is easy to understand? I am confused. Could you please do ...
Monday, September 14, 2009 at 10:12am by Mandy

Chemistry
Calculate the pH of a 50.0 mL solution 0.0120 M ethylaminium chloride (C2H5NH3Cl ) and 0.0360 M ethylamine C2H5NH2. Kb = 4.3 x 10-4 Calculate the pH when 5.0 mL of 0.1 M HI is added. Ignore any changes in the volume
Wednesday, April 17, 2013 at 12:54am by m

Chemistry
What is the pH of the solution created by combining 12.20 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? mL NaOH pH w/HCl pH w/HC2H3O2 12.20 =================================== my work: 0.000420 moles of NaOH / 0.020 ...
Monday, May 3, 2010 at 2:50pm by Amphee

Chemistry
A titration is performed by adding .600 M KOH to 40.0 mL of .800 M HCl. Calculate the pH before addition of any KOH. Calculate the pH after the addition of 5.0 mL of the base. Calculate the volume of base needed to reach the equivalence point. What is the pH at the equivalence...
Friday, April 1, 2011 at 1:18pm by Summer

Chemistry
Calculate the pH of a solute where 24.5 mL of 0.1 mol/L HCl is added to 25.0 mL of 0.1 mol/L NaOH. How much excess OH is there? .5ml .1M or 5E-5 moles. That is in a volume of 49.5ml So if OH concentration is that moles/volume, what is the H+ concentration? Remember the product...
Thursday, May 31, 2007 at 5:20pm by Raj

chemistry
NaOH + HCl ==>NaCl + HOH Strong base + strong acid. calculate mols NaOH. M x L = ?? calculate mols HCl. M x L = ?? Determine mols NaCl and HOH produced. Determine excess NaOH OR HCl and pH from that. For NaOH + HC2H3O2 ==> NaC2H3O2 + HOH Strong base + weak acid. ...
Monday, May 5, 2008 at 5:31am by DrBob22

Chemistry
mols HCl = M x L = 0.01 x 1 = 0.01 mols NaOH = 0.12 mols NaOH after neutralization = 0.11. M NaOH = M OH^- = mols/L. Then pOH = -log(OH^-) and pH + pOH = pKw = 14. Given pOH and pKw, solve for pH.
Monday, May 13, 2013 at 7:17pm by DrBob222

chemistry
How to calculate PH 1.9 = 0.0126M Why? How to calculate PH 1.8 = ? How to calculate PH 20 = ? How to calculate PH 21 = ? Pls helps me
Sunday, August 5, 2012 at 1:09pm by Fai

chemistry
1). Adding NaOH to the buret after rinsing the buret with distilled water (essentially saying that you don't rinse the buret with NaOH)means that the NaOH is more dilute so it will take more NaOH from the buret to reach the equivalence point. So more mL means mL x M = a ...
Thursday, October 1, 2009 at 7:48pm by DrBob222

chemistry
Now take another 35 mL of the 0.50 M pH 6.59 buffer and add 1.5 mL of 1.00 M NaOH. Using steps similar to those above, calculate the new pH of the solution. find pH
Monday, October 24, 2011 at 2:53pm by Taylor

Chem
25.0 mL of 0.100 M acetic acid (Ka= 1.8 x 10^-5) is titrated with 0.100 M NaOH. Calculate the pH after the addtion of 27.00 mL of 0.100M NaOH. my work CH3COOH + H2O <-> H3O^+ + CH3COO^- 25mL x 0.100 mmol/ml = 2.5mmol CH3COOH 27mL x 0.100 mmol/ml = 2.7mmol NaOH There are ...
Tuesday, June 29, 2010 at 4:02pm by Anonymous

Chemistry
I suspect the problem is that the question asks for CHANGE in pH and you're giving the data base the pH. I think something like 1.128 which I would round to 1.13 is the answer for the HCl part. I didn't work the NaOH part. pH = pKa + log(9.24/0.7). pH = pKa + 1.128. I didn't ...
Tuesday, March 27, 2012 at 6:01pm by DrBob222

Chemistry
Describe how a buffer behaves. Your description should include an explanation of why the addition of NaOH to the HAc solution formed a buffer. What happens to the pH when a small quantity of a strong acid or base is added to a buffer solution? What happens to the pH of the ...
Thursday, March 14, 2013 at 2:20am by Terrell

chemistry
The reaction between the added solid and NaOH is: NaH2PO4 + NaOH --> Na2HPO4 + H2O 10.0gNaH2PO4 /120.0g/mol = 0.0833 moles NaH2PO4 initially. In the rection, the limiting reactant is NaOH. (0.150 L)(0.20 mol/L) = 0.030 mol NaOH 0.030 moles of NaOH ---> 0.030 moles ...
Wednesday, October 7, 2009 at 8:55pm by GK

Chemistry
Take acetic acid and add NaOH to it. That produces sodium acetate, the base of the acid/base system. To make this work, one needs to use acetic acid and add NaOH but not enough to completely neutralize it. For example, if you took 10 moles acetic acid and added 5 moles NaOH, ...
Tuesday, February 14, 2012 at 5:46pm by DrBob222

Chemistry
2a. Adding 1 mL of 10M NaOH to HOW MUCH of the buffer. Since the problem gives molarities, I will assume 1L. millimols HPO4^2- = 1000 mL x 0.058 = 58 mmols H2PO4 = 1000 mL x 0.042 = 42 mmols NaOH added = 1 mL x 10M = 10 .......H2PO4^- + OH^- ==> HPO4^2- + H2O I......42...
Sunday, January 27, 2013 at 11:00pm by DrBob222

Chemistry
In one trial of an investigation 50.0 mL of HCl(aq) of an unknown concentration is Tiresias with 0.10M NaOH (aq). During the titration the total volume of NaOH (aq) added and corresponding pH value of the reaction mixture are measured and recorded in the table below: 10mL-1....
Thursday, April 14, 2011 at 5:47pm by Kelly

Chemistry
millimols HX initially = 50 x 0.06 = 3.00 mmols NaOH added for pH 5.50 = 30.0 x 0.06 = 1.8 ............HX + NaOH ==> NaX + H2O initial....3.00....0.......0......0 add...............1.8............... change.....-1.8..-1.8.......+1.8...+1.8 equil.......1.2.....0......1.8...
Tuesday, March 27, 2012 at 7:55pm by DrBob222

Chemistry
Q1: You wish to prepare a buffer solution with pH = 11.10. What volume of 6.0 M HCl would you add to 500 mL of 0.10 M (C2H5)2NH to prepare the buffer? You may assume that the solution’s volume remains constant. Q2: What is the resulting pH when 20 mL of 0.20 M NaOH is added to...
Sunday, February 24, 2013 at 1:49pm by David

Chemistry
Q1: You wish to prepare a buffer solution with pH = 11.10. What volume of 6.0 M HCl would you add to 500 mL of 0.10 M (C2H5)2NH to prepare the buffer? You may assume that the solution’s volume remains constant. Q2: What is the resulting pH when 20 mL of 0.20 M NaOH is added to...
Sunday, February 24, 2013 at 2:16pm by Anonymous

Chemistry
A titration involves titrating 0.4 M NaOH into a solution of 0.2 M H3PO4. a.) Calculate the volume of NaOH that will be required to reach the first equivalence point. b.) Calculate the volume of NaOH required to reach the second equivalence point. Other information: 10 ml ...
Saturday, February 8, 2014 at 2:03pm by Anonymous

Chemistry
One example each for 0.1M HCl/NaOH added to 25 mL H2O. The diluted HCl solution is 0.1M x (1 mL/26 mL) = (HCl) pH = -log(HCl) The diluted NaOH solution is 0.1M x (1 mL/26 mL) = (NaOH) pOH = -log(NaOH). Then pH + pOH = pKw = 14.00
Monday, March 14, 2011 at 9:32pm by DrBob222

chemistry
A 1M solution (200ml) of NH3 (Kb of ammonia=1.8*10-5) is added to 200ml of 0.5M HCl. Calculate: a) the resulting pH? b) The delta ph due to addition of 15ml of 1M HNO3 to solution obtained in part a c) I am stuck on this: The delta ph due to addition of 15ml of 1M NaOH to the ...
Thursday, February 13, 2014 at 7:05pm by anonymous

Chemistry
50.0 mL of 0.116 M NaOH is titrated with 0.0750 M HCl. Calculate the pH after the addition of 5.0 mL volume of acid.
Wednesday, May 1, 2013 at 12:33am by Nathan

chemistry
moles NaOH = grams/molar mass M = moles NaOH/L soln. (OH^-) = M NaOH pOH = -log(OH^-) Use pH + pOH = pKw = 14 to convert pOH to pH. Then convert pH to (H^+) by pH = -log(H^+).
Sunday, January 22, 2012 at 10:30pm by DrBob222

Chemistry
The secret to these problems is to know where you are on the titration curve; i.e., beginning (0 mL), equilvalence point, before the eq pt or after the eq pt. You can calculate the eq pt easily. mL acid x M acid = mL base x M base (that is always true for MONOPROTIC acids ...
Tuesday, April 23, 2013 at 1:22am by DrBob222

chem
HCl is a strong acid and ionizes 100%. NaOH is a strong base and ionizes 100%. We have no way of knowing the pH of HCl + H2O because the problem doesn't state the amount of HCl added or the concentration of HCl. For the NaOH + HCl ==> NaCl + HOH. NaCl in water is a neutral ...
Tuesday, May 15, 2007 at 5:10pm by DrBob222

Chemistry
A complicated work but do-able. NaOH + HCl ==> NaCl + H2O. I think one must decide where we are at the equivalence point. Since the M NaOH is twice that of the HCl, that means the HCl will take twice as much to neutralize the NaOH. So that 35 mL is made up of 2 mL HCl for ...
Sunday, May 2, 2010 at 11:52pm by DrBob222

Chemistry
A solution is prepared by dissolving 50.0 g of pure HC2H3O2 and 20.0 g of NaC2H3O2 in 975 mL of solution (the final volume). what is the ph? What would the pH of the solution be if 50.0 mL of 0.900 M NaOH were added? What would the pH be if 30.0 mL of 0.30 M HCl were added to ...
Monday, November 12, 2012 at 8:39pm by Bella

chemistry
if the pH of a half-neutralized acid solution is 5.4, how would you find the [H+] of the the solution. There is 1.0 g of L-ascorbic acid which was dissolved in 100 ml of water. That solution was split in two and 50 ml of the solution was titrated with 0.2 M NaOH (13 ml NaOH). ...
Thursday, April 17, 2008 at 3:04pm by tom

chemistry
What is the pH when enough 0.10 M Base NaOh (in mL) is added to neutralize 8 mL of 0.10 M Acid HCl? Acid HC2H3O2? I got the pH of HCl to be 7 because I figured that the same molarity of base and acid are added together to neutralize the pH, but I keep messing up for HC2H3O2. I...
Sunday, July 11, 2010 at 11:12pm by Sara

chemistry
HBr + NaOH ==> NaBr + H2O moles HBr = M x L moles NaOH = M x L There can be three scenarios: a. If moles HBr exactly equals moles NaOH, then you have the salt, NaBr, in water and the pH = 7 because neither Na^+ nor Br^- hydrolyze. b. If more moles HBr than NaOH are present...
Tuesday, April 27, 2010 at 5:28pm by DrBob222

Chem
Calcaulate the pH after 10.0 mL of 0.40 M HCl is added to 20.0 mL of 0.50 M NaOH. I wasnt sure on how to start this problem. I tried to break the HCl and NaOH apart then I set up ICE for each but I did get the wrong answer of 13.70. a. 0.40 b. 13.70 c. 13.30 d. 0.30
Tuesday, April 6, 2010 at 9:52pm by AMI

chemistry
moles NaOH = grams/molar mass M NaOH = moles NaOH/L solution. (OH^-) = (NaOH) pOH = -log(OH^-), then convert to pH by pH + pOH = pKw = 14'= Technically, this is not the correct answer. Technically, the correct answer cannot be obtained UNLESS one knows the density of the ...
Thursday, February 24, 2011 at 11:37pm by DrBob222

chemistry
(Re-posting because no one was answering chemistry questions) if you have 100mL of 0.1M acetic acid (ka = 1.8x10(-5)what is the pH after 10mL NaOH is added? I came up with an answer of 2.895, but i'm not sure if its right.
Thursday, October 27, 2011 at 10:15am by Kevin

Chemistry help!!
Consider the titration of the weak acid HA with NaOH. At what fraction of Ve does pH = pKa - 1? At what fraction of Ve does pH = pKa + 1? Calculate the pH at these two points plus Vb = 0, 1/2Ve, Ve and 1.2Ve, if 100 mL of 0.100 M anilinium bromide (pKa = 4.601) is titrated ...
Tuesday, November 29, 2011 at 11:01pm by Remy

Chemistry
Exactly 100 mL of 0.14 M nitrous acid (HNO2) are titrated with a 0.14 M NaOH solution. Calculate the pH for the following. (a) the initial solution (b) the point at which 80 mL of the base has been added (c) the equivalence point (d) the point at which 105 mL of the base has ...
Saturday, March 17, 2012 at 12:33am by Tanya

Chemistry
10.00 mL of an unknown base solution is titrated with .100 M HCl solution. The pH versus the volume of NaOH added is shown below. There is a graoh where there are two dotted lines signifying a pH: the highest at pH 6.31 and the lower at pH 3.92. What is the pOH pf the solution...
Thursday, March 27, 2014 at 5:58pm by Dezzi

Chemistry
Why does the addition of 50ml of 0.5M NaOH to 50mL of 0.6M KOH cause the pH to decrease (aka more acidic)? Because you have reduced the (OH^-) of the 0.6 M KOH by adding an equal volume of 0.5 M NaOH 50 mL x 0.6 M KOH = 30 millimols. pH = 13.78 Adding 50 mL x 0.5 M NaOH = 25 ...
Tuesday, August 21, 2007 at 7:34am by Vic

Chemistry
I have a test on monday and I NEED to ace it in order to raise my grade > . < ldsfkjaslkf right now, acids and bases are killing me can somebody help me with these problems? A buffer solution is prepared by mixing the weak base ammonia (Kb=1.77x10^-5) with ammonium ...
Saturday, May 15, 2010 at 2:10pm by Kimberlee

Chemistry
In a experiment to determine the molecular weight and the Ka for ascorbic acid (vit. c.) a student dissolved 1.3713g of the monoprotic acid in water to make 50 mL of solution. The pH was monitored throughout the titration. The equivalence point was reached when 35.23 mL of the...
Saturday, May 19, 2007 at 6:57pm by Tri

chemistry
Can you help me with the following: Calculate hte pH that results when 25 mL of .1M HCL is titrated with .1M NaOH solution run in from a buret at each of the stages of volume of .1 M NaOH add in 5.0 mL incrememnts beginning with 0 mL of NaOH
Friday, April 30, 2010 at 12:08pm by Cathy

chemistry
Given 1.00L of a buffer containing 0.338 M CH3COOH and 0.093 M CH3COONa. Ka(acetic acid) = 1.8 x 10-5. Calculate the pH after the addition of 0.005 moles NaOH.
Sunday, March 18, 2012 at 7:39pm by cathy

chemistry
Given 2.00L of a buffer containing 0.338 M CH3COOH and 0.093 M CH3COONa. Ka(acetic acid) = 1.8 x 10-5. Calculate the pH after the addition of 0.004 moles NaOH.
Wednesday, March 21, 2012 at 11:23pm by reichel

biochemistry
Calculate the pH change of 10mL of HCl added to 1M phosphate buffer in 1L with initil pH of 7.2?
Tuesday, September 28, 2010 at 10:08am by Lina

chem
HBr + NaOH ==> NaBr + HOH Calculate mols HBr. mols HBr = M x L = ?? Calculate mols NaOH used = M x L. Subtract mols of one from mol of the other. The one in excess will give you the H^+ if it is HBr or OH^- if it is NaOH. Then pH = -log(H^+) OR pOH = -log(OH^-)
Sunday, April 13, 2008 at 3:10pm by DrBob222

chemistry
Calculate the pH at the point in the titration of 25.00 mL 0.108 M HNO2 at which 10.00 mL 0.162 M NaOH have been added. For HNO2, Ka=5.1 x 10^-4 and: HNO2 + OH- -----> H2O + NO2- I know that HNO2 is a weak acid and that 5.1 x 10^-4=[NO2-]/[HNO2][OH-]. NaOH is a strong acid...
Sunday, October 2, 2011 at 9:42pm by Holly

chemistry
A 40.0 mL sample of 0.150 M Ba(OH)2 is titrated with 0.400 M HNO3. Calculate the pH after the addtion of the following volumes of acid, and plot the pH versus millimeters of HNO3 added. a. 0.00 mL b. 10.2 mL c. 19.9 mL d. 30.0 mL e. 39.8 mL
Monday, June 27, 2011 at 9:02pm by Cindy

Chemistry
moles acetic acid = M x L moles acetate = M x L. Add NaOH. mols added = M x L. NaOH reacts with acetic acid to produce more acetate at the expense of the acetic acid. Therefore, calulate moles NaOH added, subtract from acetic acid and add to acetate. Then M = moles/L, ...
Saturday, May 1, 2010 at 12:48pm by DrBob222

chemistry
We have two liters of a buffer solution that is 0.10 M in CH3COOH and 0.10 M in NaCH3COO. How many moles of solid NaOH are to be added to this solution to increase its pH by 5.0 percent? Assume no volume change due to the addition of solid NaOH. I have the starting pH and what...
Thursday, April 15, 2010 at 6:47pm by Bharg

Chemistry
Even if you can help answer one that would be a great help! 1. How many liters of NO(g) are produced when 0.85L of 2.00M HNO3 solution is added to 216g according to the equation. Which reactant is the limiting reactant? 3 Ag + 4 HNO3 -> 3 AgNO3 + NO + 2 H2O3 2. Calculate ...
Sunday, October 20, 2013 at 5:06pm by P.

Chemistry
I am not really sure how to do this: Calculate the pH when 1.0*10^-3 moles of solid NaOH is added to a) One liter of 9.1*10^ -6 M HCL b) One liter of a solution containig 0.05 M CH3COOH and 0.1 M CH3CooNa
Tuesday, August 11, 2009 at 7:28pm by Saira

chemistry 101
If 15g of NaOh is dissolved in 285 g of water, calculate the following. Assume the density of the solution is 1.06 g/cc. a) Calculate the moles of NaOH in the solution? My answer is 15gNaOH/40g NaOH= .0375 mole NaOH b) Waht is the mass % w/w of the solution? My answer is 15g ...
Saturday, December 8, 2012 at 12:34am by Tracy

chemistry
Lab: Determining Ka of Acetic Acid Purpose: The purpose of this experiment is to determine the molar concentration of a sample of acetic acid and to calculate its Ka. Materials: 25 mL pipet and bulb burette 2x150 mL beaker 125 mL Erlenmeyer flask acetic acid solution sodium ...
Saturday, April 5, 2008 at 12:35am by Tim's Titration Lab

chemistry laboratory
1. You don't say what the pH must be. Decide that, use pH = pKa + log(base)/(acid) and calculate the base/acied ratio, then convert to mass. 2. How many mols NaOH do you need? mols NaOH = M x L = ? mols = grams/molar mass.Solve for grams.
Thursday, May 31, 2012 at 11:48pm by DrBob222

Chemistry
A student titrates 0.025 M KOH into 50.00 ml of a solution of unknown weak acid HA. Equivalence point is reached when 30.00 ml of the KOH has been added. After 15.00ml of the KOH has been added the pH of the mixture is 3.92. A. What is the concentration of HA ? B. What is Ka ...
Thursday, March 10, 2011 at 8:18am by Patrick

Chemistry
A student titrates 0.025 M KOH into 50.00 ml of a solution of unknown weak acid HA. Equivalence point is reached when 30.00 ml of the KOH has been added. After 15.00ml of the KOH has been added the pH of the mixture is 3.92. A. What is the concentration of HA ? B. What is Ka ...
Thursday, March 10, 2011 at 1:14pm by Patrick

chem
According to my table, bromocresol green changes pH between 3.8 and 5.4. You can calculate the approximate pH for the equivalence point for CH3COOH vs NaOH and that is about 8.5 or so. What do you think?
Tuesday, November 23, 2010 at 10:13pm by DrBob222

biochemistry
The pH of 0.02M solution of a weak acid was measured at 7.6. What is the [OH-] in this solution? B) The Ka for benzoic acid is 6.4 x 10-5M. 150 ml of 0.1 M NaOH is added to 200 ml of 0.1 M benzoic acid, and water is added to give a final volume of 1 L. What is the pH of the ...
Friday, September 21, 2012 at 9:38am by Emma

chemistry
oh This is an acid base experiment this is the last stage. There are two parts: part 1) 0.3470g sodium acetate trihydate is added to 15.00 ml acetic acid (concentration is 0.20) then its mixed and a ph is taking--i got 4.30 PH part II) Added 0.7618 g of sodium acetate ...
Thursday, July 16, 2009 at 7:35pm by Jim_R

Chemistry
I have interpreted this problem differently than Bob Pursley. I think the problem states that 85 mL HCl and 89 mL NaOH WERE LEFT when the accident was discovered; therefore, we have added 100-85 = 15 mL HCl and 100-89 = 11 mL NaOH. Therefore, mmoles HCl added = 15 mL x 0.06 M...
Thursday, July 9, 2009 at 3:16am by DrBob222

Chemistry
23.55 ml of the NaOH were added to partially neutralize a new 25.00 ml sample of the acid. The pH of the mixture was measured as 5.33. Calculate Ka for the acid, HA, using the partial neutralization method
Monday, April 29, 2013 at 5:00am by GeeGee

Chem
First you must recognize that HCl is a strong acid and NaOH is a strong base; therefore, the salt produced (NaCl) will not hydrolyze and the solution will be neutral IF the HCl and NaOH EXACTLY neutralize each other. So what you need to do is to calculate the moles HCl and the...
Tuesday, April 6, 2010 at 9:52pm by DrBob222

Chemistry -- to Dr.Bob
I posted this yesterday and tried to work it out today but i don't remember how to. You said convert to moles by multiplying for example .1M x .008L= 8x10^-4 ...after this what do i do with this number to find the pH i tried to just plug that into the -log(8x10^-4) but it was ...
Friday, May 2, 2008 at 9:41pm by Amy

chemistry
a sample of 20.0 mL of 0.100 M HCN (Ka=6.2*10^-10) is titrated with 0.150 M NaOH. a) what volume of NaOH is used in this titration to reach the equivalence point? b) What is the molar concentration of CN- at the equivalence point? c) What is the pH of the solution at the ...
Tuesday, January 8, 2013 at 6:35pm by Anonymous

Biochemistry
calculate Ph occuring when 100ml of 0.10m acid is added to 500ml of 0.08m acetate buffer,pka 4.75,ph 4.5
Tuesday, August 2, 2011 at 4:25am by Pearl

Chemistry Titration Lab
Calculate the theoretical pH after 2.50 mL and 9.50 mL of NaOH has been added in both the titration of HCl and of HC2H3O2. Given: Molarity of all chemicals are 0.1 M HCl and HC2H3O2 are 8ml prepared in 100ml water. Im guessing I need to make and ICE chart but I'm having ...
Thursday, May 5, 2011 at 11:07pm by Kim

Chemistry
How does the pH of 400mL of water change when a. 100mL 0.0500M NaOH is added? b. 100mL 0.0500M HCl is added?
Monday, March 21, 2011 at 2:37am by Muffin

chemistry
You have the equation (CH3COOH = HAc; CH3COO^- = Ac^-). HAc + NaOH ==> NaAc + H2O You are starting with 0.1 M x 2 L = 0.2 mole HAc and 0.2 mole Ac^-. We want 4.982 4.982 = 4.744 + log [(Ac^-)/(HAc)] You must recognize that when NaOH is added, the HAc is decreased by x so ...
Thursday, April 15, 2010 at 6:47pm by DrBob222

chm
Write the equation and balance it. NaOH + HCl ==> NaCl + H2O Calculate moles NaOH. Calculate moles HCl. Set up an ICE chart to see what you finish with. If the moles base and moles acid are the same, they exactly neutralize each other and the pH will be exactly neutral for ...
Wednesday, March 31, 2010 at 4:20pm by DrBob222

CHEMISTRY
You subtract the moles of NaoH from the moles of HCl to determine the excess moles left, which decides the pH. To find pH, pH= -log(concent. of H+) or ( concen. of OH-) If NaOH is more than HCl, you get find pH by subtracting the pOH you get from the above formula from 14.
Sunday, October 17, 2010 at 4:50pm by Rose

Chemistry
First, the question I'm given is: What is the pH of a 1.0 L solution containing 0.25M acetic acid and 0.75M sodium acetate ( Ka for acetic acid= 1.8x 10-5) So I took the -log(1.8x10-5)= 4.74+log(.75/.25)= 5.22 pH But then I'm asked if .050 mol NaOH is added to the above ...
Monday, April 8, 2013 at 7:01pm by Marcus

chem
what color change happen when water is added to bromothymol blue indicator: a.) after addition of HCl, how does it affects the equilibrium b.) after addition of NaOH, how does it affect the equilibrium c.) after re-addition of NaOH Rewrite the net equation for the equilibrium...
Monday, November 26, 2012 at 1:53pm by kacey12

Chemistry
An unbuffered solution contaning 0.000018 M HCl .Calculate PH after adding 1 mL of 0.1 M NaOH to 100 mL of solution.
Sunday, December 11, 2011 at 8:37am by Ethio

CHEM 102
Can someone help me with this question please? What is the pH at each of the points in the titration of 25.00 mL of 0.1000 MHCl by 0.1000 M NaOH:i) After adding 25.00 mL NaOH ii) After adding 26.00 mL NaOH thankyou
Thursday, August 18, 2011 at 11:39pm by Anonymous

CHEM 102
Can someone help me with this question please? What is the pH at each of the points in the titration of 25.00 mL of 0.1000 MHCl by 0.1000 M NaOH:i) After adding 25.00 mL NaOH ii) After adding 26.00 mL NaOH thankyou
Thursday, August 18, 2011 at 11:40pm by paige

chemistry
A volume of 100mL of 1.00 M HCl solution is titrated with 1.00 M NaOH solution. You added the following quantities of 1.00 M NaOH to the reaction flask. Classify the following conditions based on whether they are before the equivalence point, at the equivalence point, or after...
Monday, August 6, 2012 at 8:00pm by Anon

Chemistry
A buffer solution is made as followed: i)adding 13.50mL of 0.200mol/L sodium hydroxide to 50.00mL of 0.100mol/L propanoic acid. ii)diluting the resulted buffer into a total volume of 100.00mL Using IRE-C tables (if possible) calculate: a)The pH of the buffer -before the ...
Monday, April 26, 2010 at 7:54am by Sara

Balthazar
A 30 ml sample of of 0.150 m hydrazoic acid (ka = 4.50x10^-4 ) is titrated with a 0.100 m NaOH what is the ph after the ff additions of NaOH 30ml 45ml 60ml
Thursday, August 1, 2013 at 2:09pm by Omi

Chem help
What is the pH of 0.000082 M NaOH? I know how to find the pH of an aqueous solution, but I'm not sure of the formula for this one... What one? Well my question was "What is the pH of 0.000082 M NaOH?," but n/m. I figured out how to do it. Thanks anyway.
Tuesday, May 22, 2007 at 10:06pm by Lindsay

Chemistry
HBr + KOH ==> KBr + HOH moles HBr initially = L x M = ? moles KOH added = L x M = ? See which is in excess and calculate pH from pH = -log (H^+). OR if mole HBr = moles KOH, the the solution has just KBr and H2O and calculate pH from that. Post your work if you need ...
Thursday, July 16, 2009 at 4:35pm by DrBob222

Chemistry
a. mol KHP = 0.4885g/molar mass = ? M = mols/0.1 L = approximately 0.024 but you need to do it more accurately. At the equivalence point the pH is determined by the hydrolysis of the P^2- ion. .........P^2- + HOH ==> HP^- + OH^- I.......0.024M...........0.......0 C...
Thursday, November 29, 2012 at 8:36pm by DrBob222

chemistry
how do you solve this What is the pH of the solution created by combining 2.60 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? mL NaOH 2.60 pH wHCl: _ pH wHC2H3O2 : _ Complete the table below: What are the pH values if you ...
Monday, July 12, 2010 at 6:03pm by Jin

Chemistry
What is the pH of 125 mL of a 1.59 M solution of a monoprotic weak acid, HA (Ka=9.53×10–5), after 29 mL of 0.37 M NaOH is added? I have no Idea how to start this problem and the homework is due tonight, could someone please help me in calculating this? Thanks
Sunday, March 31, 2013 at 5:07pm by Cory

Chemistry
A 100 milliliter sample of 0.100-molar NH4Cl solution was added to 80 milliliters of a 0.200-molar solution of NH3. The value of Kb for ammonia is 1.79 x 10^-5. (a) What is the value of pKb for ammonia? (b) What is the pH of the solution described in the question? (c) If 0.200...
Monday, April 26, 2010 at 8:49pm by Nicole

Chemistry
A 100 milliliter sample of 0.100-molar NH4Cl solution was added to 80 milliliters of a 0.200-molar solution of NH3. The value of Kb for ammonia is 1.79 x 10^-5. (a) What is the value of pKb for ammonia? (b) What is the pH of the solution described in the question? (c) If 0.200...
Monday, April 26, 2010 at 8:58pm by Nicole

chemistry
If 80g of NaOH is added to 100mL water, what is the pH of the resulting solution?
Thursday, February 24, 2011 at 11:37pm by Amy

Chemistry
Calculate the pH after 0.10 mol of HCl is added to 1.00 L of the solution that is 0.57 M HF and 1.13 M KF. I got 3.01, but it is wrong. What did I do wrong?
Sunday, March 27, 2011 at 3:04pm by Mary

chemistry
NH3 + HCl --> NH4Cl + H2O millimols NH3 = 200 x 1 = 200 mmols HCl added = 200 x 0.5 = 100 So you have 100 mmols NH3 in 400 mL solution. I assume from your post that you worked the remainder of part a. For part b we have the soln from part a and add 15 mmols (15x1) NaOH. So ...
Thursday, February 13, 2014 at 7:05pm by DrBob222

CHEM
a 250.0ml buffer solution is 0.250M in ascetic acid and 0.250M in sodium acetate. B). What is pH after addition of 0.0050mol of HCl? C). What is pH after addition of 0.0050mol of NaOH?
Wednesday, March 28, 2012 at 2:54am by ALISON

chemistry
A solution of NaOH(aq) contains 6.2 g of NaOH(s) per 100.0 mL of solution. Calculate the pH and the pOH of the solution at 25 °C.
Sunday, January 22, 2012 at 10:27pm by katie

chemistry
A solution of NaOH(aq) contains 6.2 g of NaOH(s) per 100.0 mL of solution. Calculate the pH and the pOH of the solution at 25 °C.
Sunday, January 22, 2012 at 10:30pm by katie

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