Number of results: 39,680
chemistry
a 35.5 mL sample of an NaOH solution is needed to titrate a 2.08 g sample of pure benzoic acid (HC7H5O2)a solid. What is the molarity of the NaOH solution?
Wednesday, May 9, 2012 at 10:58pm by b
Chemistry
If it takes 54 mL of 0.1 M NaOH to neutralize 125 mL of an HCI solution, what is the concentration of the HCI?
Sunday, May 12, 2013 at 10:39pm by Crystal
Chemistry
A buffer is prepared by adding 300.0 mL of 2.0 M NaOH to 500.0 mL of 2.0 M CH3COOH. What is the pH of this buffer?
Saturday, May 1, 2010 at 12:48pm by Anavia
chemistry
If 30.0 mL of 4.8 10-2 M HBr is added to 21.5 mL of 3.6 10-2 M NaOH, what is the pH of the solution?
Tuesday, April 27, 2010 at 5:28pm by Sue
Chemistry
What is the normality of 10 ml of an acid that took 25 ml of 0.25 N NaOH to reach pH 7?
Wednesday, February 17, 2010 at 1:10pm by David
Chemistry
Given PV=nRT and the following equation: CH4+2O2=CO2+2H2O Calculate the maximum number of ML of CO2 at 750 torr and 295.15 degrees K that can be formed from above conbution of methane ( CH4 ) if 450 mL of methane at 705 torr and 283.15 degrees K are mixed with 725 mL of O2 at ...
Wednesday, March 14, 2012 at 7:09pm by Chantel
chemistry
mL of 0.0100 M NaOH are added to 25.0 mL of 0.0100 M acetic acid. What is the pH of the resulting solution?
Friday, October 21, 2011 at 8:40pm by yahn
Chemistry
How much 0.10 M NaOH (in mL) is required to neutralize 8.00 mL of the 0.10 M HC2H3O2?
Sunday, May 2, 2010 at 12:57pm by John
acid and base titrations
25.00 mL of a solution of HCL was titrated with 0.4500 M NaOH using the indicator bromthymol blue. Successice readings of the burette gave the following data: colour: Volume of NaOH (mL)= i.) 16.35 yellow ii.) 16.40 yellow iii.) 16.45 green iv.) 16.50 blue Based on the data, ...
Sunday, November 21, 2010 at 5:02am by jj reddick
CHEMISTRY
Final buret reading = 31.10 Initial reading = 0 Volume NaOH = 31.10-0.0 = 31.10 mL. M NaOH = 0.2619M mols NaOH used = M x L = ? mols HC2H3O2 used = the same since this is a 1:1 reaction; i.e., NaOH + HC2H3O2 ==> NaC2H3O2 + H2O M HC2H3O2 = mols HC2H3O2/L HC2H3O2. You ...
Wednesday, March 20, 2013 at 3:58pm by DrBob222
AP Chemistry
H2A + NaOH ==> NaHA + H2O for the first H. NaHA + NaOH ==> Na2A + H2O for the 2nd H. mols H2SO4 = 0.018L x 0.122 M = ? mols NaOH = same for the first H. M NaOH = moles NaOH/L NaOH. Solve for L NaOH.
Saturday, March 17, 2012 at 2:08am by DrBob222
chemistry
Write the equation. Calculate mols HCl present Determine mols NaOH needed. Calculate mL NaOH required. Post your work if you get stuck.
Sunday, April 6, 2008 at 2:07am by DrBob222
Chemistry
If you mix 10 mL of 6 M HCl (aq) and 10 mL of 3M NaOH, will the solution be acidic, neutral, or base?
Friday, February 8, 2013 at 8:28am by Alexandria
chemistry
A buffer is prepared by adding 300.0 mL of M NaOH to 400.0 ML of 2.0 M CH3COOH. What is the pH of this buffer? ks=1.8X10^-5
Sunday, March 4, 2012 at 4:36pm by Daniel
chemistry
sorry it's: 5 mL of 0.0100 M NaOH are added to 25.0 mL of 0.0100 M acetic acid. What is the pH of the resulting solution?
Friday, October 21, 2011 at 8:40pm by yahn
Biochem
What is the pH and pOH a solution that was made by adding 400 mL of water to 350 mL of 5.0 x 10^-3 M NaOH solution?
Friday, September 2, 2011 at 1:02am by Max
chemistry
What is the molarity of an unknown acid if 40.5 ml of the acid can be titrated to an end point by 20.5 ml of 0.2250 M NaOH?
Saturday, October 16, 2010 at 5:54pm by bev
chemistry
What is the pH of the solution created by combining 12.90 mL of the 0.10 M NaOH with 8.00 mL of the 0.10 M HC2H3O2?
Monday, May 3, 2010 at 2:00pm by jc
Chemistry
A buffer is prepared by adding 300.0 mL of 2.0 M NaOH to 500.0 mL of 2.0 M CH3COOH. What is the pH of this buffer? Ka = 1.8 × 10-5
Sunday, May 2, 2010 at 10:22pm by Anavia
metro
Calculate the pH of the buffer solution that results when 10 mL of 0.10 M NaH2PO4 is added to 3 mL of 0.05 M NaOH.
Wednesday, March 17, 2010 at 12:09am by pat
chem
If 1.2 grams of sodium are reacted with 4.00 mL water, how much NaOH is produced? density of water= 1.00g/mL
Monday, September 21, 2009 at 3:47pm by Andy
Chemistry
Could someone please help me complete my lab experiment. Antacid Brand: Life Concentration of HCl: 0.1845 M Concentration of NaOH: 0.1482 M Trial 1: 1.Mass of Table: 1.2173g 2.Volume of HCl added: 75.0 mL 3.Milliomoles of HCl added:mmoles ? Help 4.Volume of NaOH used: 17.14 mL...
Monday, October 18, 2010 at 8:13pm by Akhed
Chemistry
Are you titrating the ASA with NaOH? If so use the volume NaOH in the titration. Then mols = M NaOH x L NaOH
Tuesday, June 4, 2013 at 12:29pm by DrBob222
chemisrty
A 21.00 sample of 0.3254M Hcl solution requires 26.09 ml of NaOH solution for complete neutralization. Calculate the volume of NaOH solution in liters, required for the titration.
Thursday, April 25, 2013 at 11:47am by ashley
Chemistry
To make things a little easier to type, let's realize that CH3COOH (acetic acid and written HC2H3O2) can be called HAc where H is the terminal H of the COOH and Ac stands for the remainder of the molecule. NaOH + HAc ==> NaAc + H2O moles NaOH you have. 0.1 M x 0....
Wednesday, October 28, 2009 at 8:53pm by DrBob222
chemistry
Blank corrections are useful in correcting titrations in which some unwanted side reactions occur. IN this case, measure the amount of ethanol used in the experiment, add indicator, and titrate with the NaOH until the indicator changes color. The mL NaOH added is the blank ...
Saturday, January 8, 2011 at 2:45pm by DrBob222
Introductory Chemistry
In a titration 25.1ml of a monoprotic weak acid is neutralized with 25.1 ml of .502M NaOH(aq). Calculate the Ratio of [A-] to [HA] after 12.55 of the .502 M NaOH has been added to the initial amount of HA. Anyone have any idea what's going on. I got as far as to find the ...
Wednesday, February 4, 2009 at 8:12pm by Nina
chemistry
calculate the mass of NaOH neded to prepare 500mL of a 0.10 M solution. I'm pretty sure the answer is 2g, but how do I get to that? Another question: calculate the molar amount of KHP used to neutralize the NaOH solution. .51 g of KHP was added to 50 mL of distilled H2O ...
Sunday, October 14, 2007 at 9:28pm by Rebecca
Chemistry
50 mL of 2.00 M HCl and 50 ml of 2.05 M NaOH were used
Monday, November 12, 2012 at 10:00pm by Annie
chemistry
30.0 mL of 1.50 M NaOH is diluted to 50.0 mL. What is the resulting pH?
Monday, February 28, 2011 at 3:58pm by Anonymous
Chemistry
A few questions I don't really get and need to see the work for A 50.0 mL sample of 0.55 M benzoic acid, C6H5COOH, a weak monoprotic acid, is titrated with 0.51 M NaOH. Calculate the pH at the equivalence point. Ka of C6H5COOH = 6.5 multiplied by 10-5. What is the pH of a ...
Thursday, April 22, 2010 at 1:07am by Dubs
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
Chemistry
A 50 mL sample of 8% (m/v) NaOH is diluted with water so that the final volume is 200 mL...what is the final concentration and how did you figure it out?
Monday, May 9, 2011 at 4:55pm by Curlyqty
chemistry- thank you
How much of a 0.23 M NaOH solution is needed to neutralize 27 mL of a 0.85 M sulfuric acid solution? The units are mL
Sunday, October 31, 2010 at 9:49pm by Jazmin
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
CHEMISTRRY
What is the molarity of an HCl solution if 49.0 mL is completely titrated by 68.4 mL of an NaOh solution whose concentration is 0.333 M?
Tuesday, June 8, 2010 at 3:34pm by Mel
Chem
What is the pH of the resulting solution if 30.00 mL of 0.100M acetic acid is added to 10.00mL of 0.100 M NaOH? For acetic acid, Ka=0.000018. I know that NaOH is a strong base and acetic acid is a weak acid. What is the equation: C6H5COOH+NaOH<--> C6H5COOH Once I...
Wednesday, February 27, 2008 at 4:22pm by Sarah
chemistry
My question is found in the analysis section. Thanks to all who can help 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: phenolphthalein 125 mL ...
Saturday, April 5, 2008 at 5:22pm by Kasen
Chemistry
It will take 10 mmols NaOH to convert 10 mmoles H3PO4 to NaH2PO4 and another 10 to convert to Na2HPO4 plus 5 mmoles to convert 5 mmole NaH2PO4 to Na2HPO4. That's a total of 25 mmoles needed. You hav e 0.1M NaOH, M = mmoles/mL. Substitute and solve for mL. NOTE: it's ...
Sunday, November 20, 2011 at 11:32am by DrBob222
chemistry
Hi, I posted this question earlier but still need some help: 1.3188g of antacid is weighed and mixed with 75.00mL of excess 0.1746 M HCl. The excess acid required 27.20 mL of 0.09767 M NaOH for back titration. Calculate the neutralizing power of the antacid in terms of mmol H...
Tuesday, October 5, 2010 at 11:28am by Serenity
Chemistry
You don't have enough information because I don't want to calculate anything that may use different Ksp than you have in your text/notes. Look up the Ksp fo Zn(OH)2 (Zn^2+) = Ksp/(OH^-)^2 and solve for Zn^2+ in mols/L, then M x L (100 mL or 0.1L) = mols. Then Zn^2+ + ...
Sunday, March 24, 2013 at 9:29pm by DrBob222
Chemistry-102
what is the ph solution obtained by mixing 25.00 ml of 0.250 ml HCl and 25.00ml of 0.125M NaOH
Wednesday, March 23, 2011 at 10:58pm by Christian
organic chemistry
What is the {\rm HCl} concentration if 54.2 mL of 0.100 M {\rm NaOH} is required to titrate a 30.0 mL sample of the acid?
Wednesday, December 15, 2010 at 7:28pm by casey
chemistry
if 24.25 mL of a standard M NaOH solution is required to neutralize 26.00 mL of H2SO4, what is the molarity of the acid solution?
Monday, November 3, 2008 at 10:20am by james
Chemistry
Consider a weak acid-strong base titration in which 25.0 mL of 0.100 M acetic acid is titrated with 0.100 M NaOH. a) Calculate the pH after the addition of 3.00mL of NaOH. b) What is the pH of the solution before the addition of NaOH (pKa of acetic acid=4.75) I got pH= 3.88 ...
Sunday, February 27, 2011 at 12:49pm by Jon
chem
The pH of the satd soln is 13.12; therefore, the pOH = 14 - 13.12 = 0.88 From this and pOH = -log(OH^-) you can find (OH^-) = about 0.12 (you need to do it exactly). This was diluted from 15 mL to 250 so the (OH^-) in the 250 mL flask is 0.12 x 15/250 = about 0.0072 M (again ...
Thursday, April 2, 2009 at 12:13pm by DrBob222
Chem 2068 lab
Did i get it wrong? It has KHP molar mass at 204.33 g/mol and we use 0.556 g of KHP dissolved in water. THen if 14.48 mL of NaOH is used to reach endpoint, it needs the concentration of NaOH?
Monday, October 18, 2010 at 9:12pm by Car
General Chemistry
200 mL x 0.1M H2PO4^- = 20 millimols. ?mL x 0.5M NaOH =? ........H2PO4^- + OH^- ==> HPO4^- + H2O I.......20........0..........0........0 add...............x................... C.......-x.......-x...........x E.......20-x......0...........x pH = pK2 + log(base)/(acid) ...
Thursday, January 31, 2013 at 11:05am by DrBob222
chemistry
A TUMS tablet was dissolved in 110.00 ml of 0.1022 M HCl and analyzed for CaCO3 according to the procedure described in the lab manual. It took 7.48 ml of 0.1005 M NaOH to reach the endpoint. Calculate the mass of CaCO3 in TUMS tablet to the correct number of significant ...
Wednesday, October 31, 2012 at 11:33pm by Ashley
Chemistry
What is the pH when 25 mL of .20 M CH3COOH has been titrated with 35 mL of .10 M NaOH? I got the answer .0375 but that is incorrect if you could show me steps maybe i can figure out what i did wrong thanks
Tuesday, November 30, 2010 at 10:09pm by Mya
Chemistry -- to Dr.Bob
You have too many questions within questions which makes it confusing. Let me separate the first one. What is the pH of the solution created by combining 2.30 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? NaOH + HCl ==> NaCl + HOH Strong base + strong ...
Friday, May 2, 2008 at 9:41pm by DrBob222
chemistry-buffer
How much buffer do you have? And what is the pH? 50 mL is not enough to still have a buffer after adding the NaOH to a buffer of pH = 7.55. 100 mL of the buffer with a pH = 7.55 would give a pH = 6.94 after adding the NaOH. If you need additional information, please repost at ...
Monday, February 4, 2008 at 7:01pm by drbob222
Chemisty
For clarity, just assign some number to the volume of a drop. Actually, a drop is between 0.03 and 0.05 mL (depending upon the size of the opening AND on the material that the buret/pipet/dropper is made). BUT, let's just make things simple by saying a drop is 1 mL. We ...
Wednesday, January 7, 2009 at 10:39pm by DrBob222
chemistry
The secret to these titration problems is to know where you are on the titration curve. Let's call the acid HBu. HBu + NaOH ==> NaBu + H2O mmoles HBu = M x L = 20.00 mL x 0.1 = 2 mmoles. mmoles NaOH = M x L = 26.5 mL x 0.1 = 2.65. It should be obvious that all of ...
Sunday, October 31, 2010 at 8:41pm by DrBob222
Chemistry
My calculator is on the blink; I can't do a calculation. H2SO4 + NaOH ==> H2O + NaHSO4 NaHSO4 + NaqOH ==> H2O + Na2SO4 50 mL H2SO4 x 0.5M = 25 millimoles. 50 mL NaOH x 0.50M = 25 mmols. Therefore, the first H must have been replaced and you are left with ...
Monday, April 8, 2013 at 9:45am by DrBob222
Chemistry
You prepare a solution from 10.0 mL of 0.100 M MOPS buffer (3-morpholinopropane-1-sulfonic acid) and 10.0 mL of 0.071 M NaOH. Next, you add 1.00 mL of 1.89 × 10-5 M lidocaine to this mixture Denoting lidocaine as L, calculate the fraction of lidocaine present in the form...
Wednesday, March 27, 2013 at 8:44pm by Jessica
Chemistry
You prepare a solution from 10.0 mL of 0.100 M MOPS buffer (3-morpholinopropane-1-sulfonic acid) and 10.0 mL of 0.083 M NaOH. Next, you add 1.00 mL of 5.77 × 10-5 M lidocaine to this mixture Denoting lidocaine as L, calculate the fraction of lidocaine present in the form...
Monday, February 25, 2013 at 4:09pm by Bertha
chemistry
Indicate the concentration of each ion present in the solution formed by mixing the following. (Assume that the volumes are additive.) (a) 50 mL of 0.100 M HCl and 10.0 mL of 0.510 M HCl (b) 15.0 mL of 0.309 M Na2SO4 and 38.6 mL of 0.200 M KCl (c) 3.50 g of NaCl in 40.2 mL of ...
Wednesday, September 21, 2011 at 4:09pm by Anonymous
chem 1
How much NaOH? Say 30 mL? moles NaOH = M x L = ? moles KHP = moles NaOH moles KHP = grams KHP/molar mass KHP. Solve for grams KHP
Monday, November 7, 2011 at 10:07pm by DrBob222
Analytical Chemistry
What is the cell voltage when the following volumes of 0.680 M NaBr have been added? (b) 1.0 mL (c) 13.2 mL (d) 24.7 mL (e) 25.6 mL (f) 26.0 mL (g) 38.9 mL (h) 51.4 mL (i) 52.0 mL
Thursday, April 11, 2013 at 5:51am by Micki
chemistry
How much of a 0.23 M NaOH solution is needed to neutralize 27 mL of a 0.85 M sulfuric acid solution? The units are mL. Can you please explain why you did what did Thank you
Friday, October 29, 2010 at 9:44pm by Jazmin
maths
For the reaction given below, how many grams of Na2CS3 are produced in the reaction of 65.0 mL of liquid CS2 (d = 1.26 g/mL) and 1.56 mol NaOH?
Tuesday, September 21, 2010 at 4:06pm by srujan
chemistry
The cola sample is 50. mL, the equivalence point volume is 13.4 mL, and the NaOH solution concentration is 0.025 M, what mass of H3PO4 was in the sample?
Wednesday, August 11, 2010 at 8:43pm by Kris
chemistry
It took 7.5 mL of 2.8 x 10^-3 M NaOH so that is M x L = moles HCl. You have that many moles H^+ in the 300 mL sample of water; therefore, divide mole/L = M = concn H^+.
Thursday, March 26, 2009 at 10:26pm by DrBob222
chemistry
25 mL of standardized 0.45 mol/L NaOH is titrated with 21 mL of 0.35 mol/L acetic acid. Calculate the pH of the solution
Wednesday, April 9, 2008 at 9:26pm by unknown
Chemistry
When a diprotic acid, H2A, is titrated by NaOH, the protons on the diprotic acid are generally removed one at a time, resulting in a pH curve that has the following generic shape. (a) Notice that the plot has essentially two titration curves. If the first equivalence point ...
Thursday, March 7, 2013 at 9:57pm by Franklin
chemistry
Assuming the temperature and pressure are held constant, which of the gas samples has the greatest number of gas particles? Answer 45.0 mL O3 35.0 mL N2 15.0 mL of CO2 25.0 mL of SO3 how would i go about answering this question.
Saturday, January 19, 2013 at 1:26am by jakey
CHemistry
im not sure how u solve these types of problems... How many moles of NaOH are contained in 200ml of a 0.1M of NaOH? How many grams of NaOH are contained in 500ml of a .5M solution of NaOH? <<How many moles of NaOH are contained in 200ml of a 0.1M of NaOH? >...
Saturday, April 21, 2007 at 10:21pm by Phil
chem
millimols HF = mL x M = 500 mL x 0.43M = 215 mmols F^- = 500 mL x 0.45M = 225 40 mL x 0.1M NaOH = 4 millimols. ...........HF + OH^- ==> F^- H2O initial...215....0......225...... add.............4.0............ change...-4.....-4........+4......... equil....211......0...
Thursday, April 19, 2012 at 9:19pm by DrBob222
Chemistry
A very old and tired , grey haired AP Chem instructor wanted to determine the Ka of an unlabelled monoprotic acid in his stockroom. He dissolved an unknown amount of acid in an unknown amount of water and proceeded to titrate the sample with a solution of NaOH of unknown ...
Sunday, February 24, 2013 at 9:19pm by Summer
Chemistry
A very old and tired , grey haired AP Chem instructor wanted to determine the Ka of an unlabelled monoprotic acid in his stockroom. He dissolved an unknown amount of acid in an unknown amount of water and proceeded to titrate the sample with a solution of NaOH of unknown ...
Sunday, February 24, 2013 at 8:42pm by Kat
chemistry
2NaOH + H2SO4 ---> Na2SO4 + 2H2O n = (Molarity)(vol) n= (0.10M)(0.04L) =0.004moles of H2SO4 0.004molesH2SO4 * 2moles NaOH/1mole H2SO4 = 0.008moles NaOH so M= n/v v=n/M = 0.008/0.50 = 0.004L 0.004*1000 = 4.0 ml
Saturday, March 6, 2010 at 4:43pm by Zoey
Chemistry
H2SO4 + 2NaOH ==> 2H2O Na2SO4 mol NaOH = grams/molar mass Convert mols NaOH to mols H2SO4. That will be mols H2SO4 = 1/2 mols NaOH. M H2SO4 = mols H2SO4/L H2SO4. You know M and mols, solve for L H2SO4 and convert, if you wish, to mL.
Monday, October 8, 2012 at 6:11pm by DrBob222
Chemistry
got NaOH+KHC8H4O4-->H2O+KNaC8H4O4 is this correct? yes •Name the secondary standard used in the titration of the unknown KHP mixture. NaOH • Calculate the amount of NaOH (in millimoles) delivered in the titration. mL x M = millimols • Find the mass of KHP...
Wednesday, March 7, 2012 at 3:58pm by DrBob222
Chemistry
Calculate the pH at the halfway point and at the equivalence point for each of the following titrations. (a) 100.0 mL of 0.14 M HC7H5O2 (Ka= 6.4 multiplied by 10-5) titrated by 0.14 M NaOH halfway point equivalence point (b) 100.0 mL of 0.29 M C2H5NH2 (Kb = 5.6 multiplied by ...
Friday, June 1, 2012 at 5:13pm by Andrew
Chemistry
A mass of 0.4113 g of an unknown acid, HA, is titrated with NaOH. If the acid reacts with 28.10 mL of 0.1055 M NaOH, what is the molar mass of the acid?
Saturday, April 28, 2012 at 2:23pm by Tiffany
Chemistry
The pH of a weak monoprotic acid, HA, is 4.55. It took 39.22 ml of 0.2334 M NaOH to titrate 25.00 ml of the acid. a. Write an equation for the above reaction. b. Calculate the molarity of the weak acid c. Write the equilibrium equation. Construct a table showing initial ...
Saturday, April 9, 2011 at 2:54pm by Cassie
chemistry
molarity = moles/L moles = g/molar mass So 25 g NaOH is how many moles? You place that in 150 mL water (0.150L) and the molarity is what? Then (NaOH) = OH^-. Convert that to pOH, then to pH.
Sunday, April 18, 2010 at 8:36pm by DrBob222
chem
What is the pH of the solution created by combining 2.40 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)? I understand how to find the pH for the NaOH + HCl solution. However, I'm not sure how to find it for HC2H3O2. I ...
Monday, May 2, 2011 at 8:10pm by Anonymous
Chemistry
Sorry I nee to add something. The Ka for HF = 1 x 10^-3. Is 50.0 mL of 1.0 M HF and 25.0 mL of 1.0 M NaOH a buffer with an approximate pH of 3? I say yes. Right?
Thursday, May 6, 2010 at 2:15pm by Jim
science
i better write it out properly Naoh=2.991 mol Hcl=25.00 Ml, Density =0.952g/ml, mm=35.46g/mol
Tuesday, September 1, 2009 at 1:08am by Jim_R
Science
We conducted an expirement to detect disulphide groups in protein. One tube(lysozyme) contained unkowns, had approx 9.34 micromoles of disulphide groups. The question asks me to work backwards through all the dilution factors taken to give number of micromoles of disulphide ...
Thursday, March 29, 2012 at 2:48pm by Shri
Chemistry
#1. For H2SO4L: 2NaOH + H2SO4 --> Na2SO4 + 2H2O moles H2SO4 = M x L = ?? moles NaOH = 2x moles H2SO4 (from the equation). M NaOH = moles NaOH/L NaOH. #1. For HCl: NaOH + HCl ==> NaCl + H2O moles NaOH = M(from the first part) x L moles HCl = moles NaOH (from the ...
Monday, October 4, 2010 at 3:03pm by DrBob222
Chemistry
If 18.7 mL of 0.14 M MgCl2 are mixed with 24.2 mL of 0.52 M NaOH, what will be the final concentration of Mg2+ in solution when equilibrium is established? Assume the volumes are additive. Ksp = 1.2 10-11 for Mg(OH)2.
Thursday, March 14, 2013 at 11:38pm by Arturo
chemistry
As from the equation the ratio is 1:1 Use M1V1=M2V2 (i.e. working in mmoles) thus 43.50 ml x 0.105 M (NaOH) = 5.00 ml x X where X is the molarity of the vinegar and taek care with the sig figs.
Monday, October 31, 2011 at 7:22am by Dr Russ
Chem 2 Lab
H3PO4 + 3NaOH ==> 3H2O + Na3PO4 mols H3PO4 = 0.4/molar mass H3PO4 = ? Convert mols H3PO4 to mols NaOH using the coefficients in the balanced equation. M NaOH = mols NaOH/L NaOH. You know M and mols NaOH, solve for L NaOH
Wednesday, April 25, 2012 at 10:30pm by DrBob222
AP Chemistry
A very old and tired , grey haired AP Chem instructor wanted to determine the Ka of an unlabelled monoprotic acid in his stockroom. He dissolved an unknown amount of acid in an unknown amount of water and proceeded to titrate the sample with a solution of NaOH of unknown ...
Sunday, February 24, 2013 at 2:42pm by Sarah
Chemistry
3.30 mL of vinegar needs 40.0 mL of 0.150M NaOH to reach the equivalence point in a titration, how many grams of acetic acid are in a 1.10 qt sample of this vinegar?
Thursday, June 28, 2012 at 11:24pm by Aaron
chem
A hydrofluoric acid buffer solution has the following concentrations: [HF]=0.43M [F-]=0.45M If 40 mL of 0.1M NaOH is added to 500 mL of the buffer, what is the resultant pH?
Thursday, April 19, 2012 at 9:19pm by Jess
chemistry
3.30 mL of vinegar needs 43.0 mL of 0.150 M NaOH to reach the equivalence point in a titration, how many grams of acetic acid are in a 1.70 qt sample of this vinegar?
Wednesday, February 29, 2012 at 7:09pm by karen
Chemistry
Construct the data chart and the pH curve for the titration of 25 mL of 0.1 M CH3COOH with 0.1M NaOH. Add the titrant 1 mL at a time and calculate the pH after each addition
Tuesday, April 19, 2011 at 12:28am by Jake
Science
A 10 mL sample of tartaric acid (a diprotic acid) is titrated with 20 mL of 1.0 M NaOH. What is the molarity of the acid?
Thursday, December 29, 2011 at 7:20am by Fahmi
chemistry
If 5.00 mL of HCl require 4.03 mL of 0.9581 M NaOH to just consume the HCl, what is the concentration of the HCl?
Sunday, July 25, 2010 at 2:58pm by Ellen
Chemistry
If 5.00 mL of HCl require 4.59 mL of 0.9581 M NaOH to just consume the HCl, what is the concentration of the HCl?
Monday, February 22, 2010 at 5:37pm by Caryn
chem
15% w/w means 15 g H2SO4/100 g solution. That's 15 g H2SO4/(15 g H2SO4 + 85 g H2O) BUT that doesn't tell us the volume of that 100 grams of solution. I don't know how much solute is in 500 mL because I don't know what 500 mL weighs. You need the density of the ...
Thursday, November 29, 2012 at 10:51am by DrBob222
Chem
Tt is found that an average volume of 24.25 ml of approximately 0.1 M NaOH is required to reach an endpoint in a titration with 25.00ml of 0.09917 M HCl solution. What is the NaOH concentration? Make sure to give answer to four significant figures.
Friday, May 3, 2013 at 1:11am by Abenaa
College Chemistry
......H2PO4^- + OH^- ==> HPO4^-2 + H2O start..23.75 .....0.........0.........0 change..-x........x.........x.........x end...23.75-x.....0........x...........x Substitute this into the (B/A) = 0.5036 equation below. [mmoles H2PO4 at start is from 125 mL x 0.19 M = 23.75...
Saturday, November 20, 2010 at 2:08pm by DrBob222
chemistry
Transfer the tablet to a clean 125-mL Erlenmeyer flask. Add 10-mL of 1M NaOH and heat the mixture to a gentle boil. Once the solution has cooled to room temperature, transfer it to a 100-mL vol. flask. Using the diluted solution from the 100-mL volumetric flask, rinse a 1-mL ...
Sunday, January 31, 2010 at 7:20pm by eng
Chemistry
The flask shown contains 10.0 mL of HCl and a few drops of phenolphthaein indicator. The buret contains 0.270 M NaOH. What volume of NaOH is needed to reach the end point of the titration? What was the initial concentration of HCl?
Monday, November 22, 2010 at 7:02pm by Jason
Chemistry
compute volume and/ or weights of reagents to make the following solution. Desired concentration: 40% NaOH + 4% Na2S2O3 Desired quantity: 1500 mL Given: 90% w/w NaOH, pure Na2S2O3 I'm not sure how to do this so any help would be great. Thanks!
Monday, September 17, 2007 at 8:33pm by Alan
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