Sunday
March 9, 2014

# Search: diluted pH

Number of results: 7,355

chemistry
You want total moles of M x L. Then moles = grams/molar mass. Solve for grams. Are you sure about 3.16 x 10^-4? Plug that back into Ka = x^2/(3.16e-4-x) and see if you get pH of 3.5. In fact, a H^+ of 3.16 x 10^-4 gives you a pH of 3.5 (what you want); however, the question ...
Wednesday, October 6, 2010 at 8:55pm by DrBob222

CHEMISTRY/
A student takes a 1.00 mL aliquout of 5.00*10^-4 M HCl solution and dilutes it to the mark with water in a 1000.0 mL volumetric flask. (a)What is the expected pH for the final solution at 25C? (b)What would be the expected pH if this solution were later used at a temperature ...
Sunday, March 20, 2011 at 5:38am by TORI

Chemistry
I need to find the tested and published pH values of the following solutions: (1) 1.0 M NaCl (2) 1.0 M sodium acetate (3) 1.0 M sodium sulfate (4) 1.0 M Sodium Bisulfate (5) 1.0 M Sodium Carbonate (6) 1.0 M Ammonium Chloride\ Is there a reliable MSDS program, I can find the pH...
Tuesday, March 6, 2012 at 7:44pm by Really Need Help

Biology
I did a lab biology project on seed germination and the results weren't as expected. pH 5 worked better than pH 6 or 7 which seemed weird because surely it would be too acidic. I've been trying to find an explanation as to why I got these results and I think, possibly, it's to...
Sunday, January 11, 2009 at 2:51pm by Anonymous

Biology
I did a lab biology project on seed germination and the results weren't as expected. pH 5 worked better than pH 6 or 7 which seemed weird because surely it would be too acidic. I've been trying to find an explanation as to why I got these results and I think, possibly, it's to...
Sunday, January 11, 2009 at 4:22pm by Anonymous

AP CHEMISTRY
A buffer, consisting of H2PO4− and HPO42−, helps control the pH of physiological fluids. Many carbonated soft drinks also use this buffer system. What is the pH of a soft drink in which the major buffer ingredients are 7.20 g of NaH2PO4 and 4.90 g of Na2HPO4 per ...
Saturday, March 3, 2012 at 4:25pm by MARY

AP Chemistry
A buffer, consisting of H2PO4− and HPO42−, helps control the pH of physiological fluids. Many carbonated soft drinks also use this buffer system. What is the pH of a soft drink in which the major buffer ingredients are 7.20 g of NaH2PO4 and 4.90 g of Na2HPO4 per ...
Monday, March 12, 2012 at 6:42pm by HELP PLEASE

science
I added 40 mL of NaOH 1N to rise the pH of 10g teriphitalic acid from 5.3 to 6.3, so if I adde the same 40 mL of NaOH to 12g of the same acid what is the new pH will I have?
Friday, January 22, 2010 at 4:06pm by Jack

For Dr.Bob222 (chem work)
Almost. 0.15 mol/L * 0.12 L = 0.018 mol acetic acid OK 0.2 mol/L * 0.03 L = 0.006 mol NaOH OK 0.018 - 0.006 = 0.012 mol of acetic acid in excess very good pH = pKa + log (acid/base) The next step is where you went wrong. 0.006 is the number of mol of base (acetate ion) formed...
Monday, August 27, 2007 at 11:17pm by DrBob222

Chemistry (Acids and Bases)
I just did a lab on Acids and Bases and I am having trouble with the lab questions I was given to complete. Concentration of NaOH: 0.09999 M Volume of NaOH: 3.25 mL # moles of NaOH: 0.325 moles Initial Concentration of Weak Acid: ? (How do we calculate this) Part 2: Hydrolysis...
Sunday, March 29, 2009 at 1:54pm by Lalu

Chemistry
I don't know how advanced you class is but I would offer two or three suggestions. 1. The temperature of the water was not 25 C where Kw for H2O is 1.008E-14. 2. The ionic strength of the solution was not taken into account. 3. The water used for the experiment had CO2 (from ...
Saturday, March 2, 2013 at 10:05pm by DrBob222

science
A student prepared a .10M solution of acidic acid. Acidic acid has a Ka of 1.75 x 10-3. What are the hydronium ion concentration and the PH of the solution? I think the PH is 1.76 because I hit -log(1.75 x 10-3) on my calculator and thats what I got thanks in advance for your ...
Wednesday, March 21, 2007 at 4:21pm by Jodi

A bottle of 12.0 M hydrochloric acid has only 35.7 mL left in it. What will the HCl concentration be if the solution is diluted to 250.0 mL?
Sunday, September 29, 2013 at 6:17pm by Alexandra

Chemistry
Our teacher asked, a few weeks ago, for us to find the pH of 7.65 E-11 M HClO3. We were told that we couldn't find the pH simply by -log[7.65E-11]. He said that we had to account for the water somehow [I think we had to do something with the number 1.0 E-7]. Does anyone know ...
Sunday, May 20, 2007 at 5:46pm by Krystal

Chemistry
Henderson-Hasselbalch equation: pH=pKa+log((base)/(acid)) Kb*Ka=1.0*10^-14 1.74*10^-5*Ka=1.0*10^-14 Ka=1.0*10^-14/1.74*10^-5 Ka=5.75*10^-10 pKa=-log(5.75*10^-10) pKa=9.24 pH=9.24+log((.246)/(.0954)) pH=9.65
Sunday, April 15, 2012 at 6:55am by Whitney

Chemistry
When the concentration of a weak acid in solution is equal to the concentration of its conjugate base in solution, then: Would pH=pKa or would it equal pH=pKa + 1 like Henderson-Hasselbalch equation?
Sunday, April 7, 2013 at 6:01am by Marcus

Biochemistry
HCl is completely ionized. So, one gets one H+ for each HCl molecule. The concentration of HCl is .2M, so the concentration of the H+ is .2M Then, the defintion of pH pH= - log .2= you do it.
Wednesday, January 23, 2008 at 8:04pm by bobpursley

chemistry
"Taking 1/2 the volume at the equivalence point and reading the pH at that point will give you the pKa of the acid." Do you mean reading the pH at that point will give me the Ka* of the acid?
Tuesday, April 8, 2008 at 11:39pm by Anonymous

Chemistry
3.a solution has 64 grams of HI dissolved in 250 L of water. what is its [H+] 4. What is the pH of the solution in question #3? 5. A solution has 189 grams of HNO3 dissolved in 1000 L of water. What is pH?
Tuesday, February 25, 2014 at 12:23pm by Emma

chem
A beaker with 120mL of an acetic acid buffer with a pH of 5.00 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 5.70mL of a 0.450M HCl solution to the beaker. How much will the pH change? The pKa of acetic acid ...
Monday, July 22, 2013 at 3:50pm by pablo

Chem
Given that Kw = 2.4x10^-14 at 37 celsius, compute the PH of a neutral aqueous solution at 37 celsius, which is the normal human body temperature. Is PH = 7 solution acidic, basic, neutral at 37 celsius? Thank you!!!!!!
Saturday, October 9, 2010 at 7:51pm by Kim

Chemistry
mols NaOH = grams/molar mass M NaOH = mols/L solution. L soln = 0.1 L in the problem. Then (OH^-) = (NaOH) pOH = -log(OH^-) pH + pOH = pKw = 14. You know pOH and pKw, solve for pH. Post your work if you get stuck.
Saturday, October 19, 2013 at 8:25pm by DrBob222

chemistry
What mass in grams of potassium hydroxide is contained in 500 mL of solution that has a pH of 11.5? Your response: [OH] = 1.0 x 0^-14 / 11.5 This isn't correct. If the pH is 11.5, then the pOH = 14 - 11.5 = 2.5 = pOH and (OH^-) = 0.00316 M. It appears to me that you have Kw ...
Monday, April 7, 2008 at 5:01pm by Dustin

chem
2HNO3 + Ba(OH)2 ==> 2H2O + Ba(NO3)2 mols HNO3 = M x L = ? Use the coefficients to convert mols HNO3 to mols Ba(NO3)2. mols Ba(OH)2 = M x L = ? Convert mols Ba(OH)2 to mols Ba(NO3)2. It is likely you will obtain two different numbers for mols Ba(NO3)2 so one of them must be ...
Tuesday, November 13, 2012 at 2:08pm by DrBob222

Chem
You need to have two pieces of information before applying the dilution formula. 1. You need to convert pH to M. pH = -log(H^+) 2.13 = pH. I get (H^+) = approximately 0.007 but you need to do that more accurately. 2. You need to convert 36% HCl to molarity. density = 1.18; ...
Monday, February 28, 2011 at 1:50am by DrBob222

algebra
Part 1: Using the Library, web resources, and/or other materials, find the logarithmic formula that gives the pH of a substance. State what each variable in your equation represents. Find the pH of an acidic substance of your choice. Using this pH, show how to find the ...
Tuesday, December 8, 2009 at 10:59pm by steph

algebra
Part 1: Using the Library, web resources, and/or other materials, find the logarithmic formula that gives the pH of a substance. State what each variable in your equation represents. Find the pH of an acidic substance of your choice. Using this pH, show how to find the ...
Friday, December 11, 2009 at 8:08pm by stephanie

Chemistry
I can't draw on this forum how these things look; however, remember that with the HA, adding NaOH produces a buffered solution. Because it's a weak acid the initial pH (before any NaOH is added) is higher and the addition of NaOH forms NaA. The mixture of unreacted HA and the ...
Thursday, March 3, 2011 at 11:10pm by DrBob222

Chemistry, #1
At 40 degrees C, the value of Kw is 2.92 x 10^-14. a)Calculate the [H+] and [OH-] in pure water at the same temperature. b)What is the pH of pure water at that temperature? I know how to do this with Kw being 1.0 x 10^-14 at 25 degrees C, but how do I do this with a different ...
Friday, August 3, 2007 at 4:10pm by Taasha

Buffer solution
Solve an equilibrium problem (using an ICE table) to calculate the pH. a solution that is 0.205 M in CH3NH2 and 0.110 M in CH3NH3Br. i used th Ka of CH3NH2 and set up the problem as Ka=[H3O][CH3NH2]/[CH3NH3Br], but that was wrong. So i switched the equation to Ka=[H3O][...
Saturday, March 27, 2010 at 7:34pm by Kyle

Chemistry
A solution contains 0.0273 M HNO3, 0.0302 M HI, and 0.320 M formic acid, HCOOH. What is the pH? A solution contains 0.160 M Ba(OH)2 (strong base) and 0.360 M ammonia, NH3 (weak base). What is the pH? I'm really not sure how to do this. I tried and got .443 and 12.91 ...
Saturday, March 2, 2013 at 4:59pm by Anonymous

chemistry
Calculate the pH at the equivalence point for the titration of a solution containing 1250.0 mg of hilariamine (MW = 92.5 g/mol, Kb = 8.1×10−4) with 0.1000 M HCl solution. The volume of the solution at the equivalence point is 175.0 mL. (I got the answer to be 12.0208 but...
Sunday, May 15, 2011 at 8:02pm by vivian

chemistry
Calculate the pH at the equivalence point for the titration of a solution containing 1250.0 mg of hilariamine (MW = 92.5 g/mol, Kb = 8.1×10−4) with 0.1000 M HCl solution. The volume of the solution at the equivalence point is 175.0 mL. (I got the answer to be 12.0208 but...
Sunday, May 15, 2011 at 8:02pm by vivian

Chemistry
I would calculate all of them but that doesn't take into account all of the variables. I don't know of any program (computer program that is) nor group. Frankly, I think you could make up these six solutions fairly quickly, then measure them with a pH meter IF (and that's a ...
Tuesday, March 6, 2012 at 7:44pm by DrBob222

Chemistry
What is the pH of a buffer solution that is made by adding 21.0 grams of sodium fluoride to 1.00 Liter of 0.15M hydrofluoric acid? (see the Table above for the Ka of hydrofluoric acid; calculate the pH to 2 decimal places) hint: you will have to find the molarity of NaF in ...
Monday, June 17, 2013 at 10:36pm by D.J.

Chemistry
what is the resultig pH if 0.005 mol of NaOH is added to 100.0mL of buffer containing 0.010 mol acetic acid (CH3COOH,pKa = 4.74)and 0.010 mol sodium acetate (NaCH3COO)? (Assume the final volume is 100 mL) So i worked it out, i just need to double check the pH. Let me know what...
Tuesday, October 22, 2013 at 12:05am by Kyle

Chemistry
What is the pH of a 0.1 M NaOCl solution (Ka of HOCl is 2.95 x10-8) I did: x squared/.10= 2.95x10-8 x squared= 2.95x10-9 x= 5.43x10-5 -log(5.43x10-5)= 4.27 pH However, the options I'm given are either a.) 3.74 b.) 6.47 c.) 8.23 d.) 10.27 What steps am I doing wrong?
Monday, April 8, 2013 at 7:08pm by Marcus

CHEMISTRY
Solution A has pH of 4.6 and solution B has a pH of 8.0 1- What is the (H3O+) in solution A? 2- What is the (OH-) in solution B ?
Thursday, June 3, 2010 at 8:56pm by Lynne

Chemistry
pH = pKa + log(base)/(acid) Plug in pH you want, plug in pKa for NH3 (that will be Kw/Kb since you can't find the Ka listed in any table), you're given NH3 (make up a volume for that and enter moles), solve for (NH4Cl). Convert to grams in the volume you chose for the NH3.
Sunday, March 4, 2012 at 10:42pm by DrBob222

Chemistry
To what volume must a solution of 86.1 g H2SO4 in 494.0 mL of solution be diluted to give a 0.18 M solution?
Wednesday, May 11, 2011 at 12:26am by Sam

chem
Help with this one please? If you place a piece of blue litmus paper in 200mL of dilute hydrochloric acid, the litmus paper turns pink. If you then add 2 drops fo phenolphthalein, the solution remains coloreless. If you add a few drops of dilute calcium hydroxide solution, the...
Tuesday, May 15, 2007 at 8:23pm by Horacio

Chemistry
pH x = 4.35; therefore, pOH = 9.65 y has 10x higher OH; therefore, pOH must be 8.65 which makes pH = 14-8.35 = 5.35 z is 4.35 + 4.0 = 8.35 You can change these to H^+ and calculate the ratio and classify as acid, base, neutral.
Tuesday, March 19, 2013 at 2:12pm by DrBob222

chemistry
(10 Points) A water initially contains 50 mg/L of Mg 2+ The pH of the water is increased . until the concentration of hydroxide ion is 0.0005 M. Calculate the concentration (mg/L) of magnesium ion in this water at this pH. Assume that the temperature of the solution is 25˚C
Wednesday, February 23, 2011 at 3:03am by Jazmin

Chemistry
Any combination of acid and base titration will give a SHARP end point caused by a large increase (or decrease depending upon what is titrating what) of about 4 or 5 pH units EXCEPT for the titration of a weak acid with a weak base. With the WA/WB titration it is essentially ...
Thursday, May 12, 2011 at 7:28pm by DrBob222

Biochemistry DR.BOB
Isn't a phosphate buffer @ pH about 7.2 composed of NaH2PO4 and Na2HPO4? So you must add enough NaOH to completely neutralize the first hydrogen; therefore, you add 100mL x 0.1M mmoles NaOH to START. Then calculate the base(HPO4--/H2PO4-) you need to ADD to the NaOH initially ...
Tuesday, February 1, 2011 at 5:30pm by DrBob222

Chemistry
Phosphoric acid, H3PO4(aq), is a triprotic acid, meaning that one molecule of the acid has three acidic protons. Estimate the pH, and the concentrations of all species in a 0.300 M phosphoric acid solution. kPa1: 2.16 kPa2: 7.21 kPa3:12.32 [H3PO4] = ? [H2PO4-] = ? [HPO42...
Sunday, March 10, 2013 at 2:47pm by Paula

Chemistry
Phosphoric acid, H3PO4(aq), is a triprotic acid, meaning that one molecule of the acid has three acidic protons. Estimate the pH, and the concentrations of all species in a 0.100 M phosphoric acid solution. pKa1 = 2.16 pKa2 = 7.21 pKa3 = 12.32 [H3PO4] = ? [H2PO4-] = ? [HPO42...
Tuesday, February 26, 2013 at 7:21pm by Nancy

Chemistry
how do I find the pH of a buffer solution given that 0.010M NH3 mixed with 0.0030M NH4Cl. Also... a 0.010M HF solution is mixed with 0.030M KF. FIND THE pH of this mixed solution.
Sunday, March 25, 2012 at 9:03pm by Declan

Chemistry
The pK3 of formic acid is 3.75 A)what is the pH of a buffer in which formic acid and sodium formate have equimolar concentration? B)what is the pH of a solution in which the sodium formate is 10M and the formic acid is 1M?
Tuesday, April 30, 2013 at 1:50pm by Liz

chemistry
You diluted a bacterial culture 106, plated out 200 µL and found 38 colonies on the plate. How many bacteria/mL were in the original undiluted culture?
Tuesday, September 13, 2011 at 1:36pm by nicky

Chemisty
25.0 mL of 0.250 M MgCl is transferred to a 300.0 mL volumetric flask and diluted to the mark with deionized water. What is the concentration of the dilute solution?
Tuesday, April 10, 2012 at 6:36pm by Wyatt

science
You end up with ten times as much H2O and the same amount of NaOH. That makes a 0.2M solution. You have diluted by a factor of ten.
Thursday, August 16, 2012 at 10:02pm by drwls

Chemistry- acids/bases
Find the concentration of OH- of a solution of 45.0mL of 0.0921 M Ba(OH)2 diluted with enough water to make 350.0 mL of solution.
Wednesday, February 12, 2014 at 7:13pm by Jessica

Chemistry- acids/bases
Find the concentration of OH- of a solution of 45.0mL of 0.0921 M Ba(OH)2 diluted with enough water to make 350.0 mL of solution.
Wednesday, February 12, 2014 at 7:14pm by Jessica

Chemistry
I have 500 mL of a 6.0 M solution that I want diluted down to 2 M. How many mL of water should I add to the solutiion. " FOR EVERY PROBLEM YOU MUST DRAW A PICUTRE"
Thursday, February 20, 2014 at 6:18pm by Emma

Chemistry
if 25.0 mL of 15M nitric acid is diluted to 125 mL, what is the concentration of the new solution? i got 3M but i dont think its right
Tuesday, March 4, 2014 at 6:37pm by Anonymous

Chemistry
if 25.0 mL of 15M nitric acid is diluted to 125 mL, what is the concentration of the new solution? i got 3M but i dont think its right
Tuesday, March 4, 2014 at 7:07pm by Anonymous

college chem
To solve this, you require the Henderson-Hasselbach equation: pH = pKa + log(conc.base/conc. acid) You have pH and pKa, so plug in the numbers, and solve for the ratio of Base/acid. With some algebra, you can then figure out the volume amounts of each species.
Tuesday, March 23, 2010 at 11:54pm by Chris

Chem 2
Checking to see if I did this right? Titration of HN03 titrated with NaOH ending result is 1.38. Titration A, endpoint pH = 8 is pKa or pKb= 1.38x106=5.861 and Titration of NH03 titrated with KOH ending results 1.54. Titration B, endpoint pH = 7 is KaorKb= Ka=1.54x105
Wednesday, March 21, 2012 at 11:58pm by Debbie

Science
C6H5NH2 + H2O C6H5NH3+ + OH- 1. Aniline, a weak base, reacts with water according to the rxn above. a. A sample of aniline is dissolved in water to produce 25.0 ml of a .10 M soln. The pH of soln is 8.82. What is Kb for this rxn? b. The soln in part b, is titrated with...
Saturday, April 12, 2008 at 6:27pm by Francis

Chemistry
Can you explain what you don't understand here? The first thing you do is calculate where the equivalence point is. A is just calculation of pH of a weak acid. Then you have all of the calculations leading up to the eq. pt, all of the calculations after the eq. pt. and finally...
Sunday, February 10, 2013 at 5:35pm by DrBob222

Quantitative Analysis
The dibasic compound B (pKb1 = 4.00, pKb2 = 8.00) was titrated with 1.00 M HCl. The initial solution of B was 0.100 M and had a volume of 100.0 mL. Find the pH at the following volumes of acid added and make a graph of pH versus Va; Va=0, 1, 5, 9, 10, 11, 15, 19, 20, and 22mL.
Wednesday, November 14, 2012 at 12:21pm by Missy

chemistry
The skeletal structures of the two amino acids, glycine and lysine, are given below along with the values of the relevant acid dissociation constants (pKa). (a) For an aqueous solution of glycine alone, calculate the value of pH at which the ratio of the concentration of ...
Saturday, June 1, 2013 at 8:19am by a

chemistry
What is the pH of a buffer solution that is made by adding 21.0 grams of sodium fluoride to 1.00 Liter of 0.15M hydrofluoric acid? (see the Table above for the Ka of hydrofluoric acid; calculate the pH to 2 decimal places) hint: you will have to find the molarity of NaF in ...
Sunday, June 16, 2013 at 6:17pm by dennis

chemistry
What is the pH of a buffer solution that is made by adding 21.0 grams of sodium fluoride to 1.00 Liter of 0.15M hydrofluoric acid? (see the Table above for the Ka of hydrofluoric acid; calculate the pH to 2 decimal places) hint: you will have to find the molarity of NaF in ...
Sunday, June 16, 2013 at 6:17pm by Dennis

chemistry
What is the pH of a buffer solution that is made by adding 21.0 grams of sodium fluoride to 1.00 Liter of 0.15M hydrofluoric acid? (see the Table above for the Ka of hydrofluoric acid; calculate the pH to 2 decimal places) hint: you will have to find the molarity of NaF in ...
Sunday, June 16, 2013 at 9:41pm by Dennis

Chem 111
A solution is prepared by mixing 499 mL of 0.19 M Tris·Base and 592 mL of 0.37 M Tris·Acid. What is the pH of this solution? [Ka(Tris·Acid) = 8.5 × 10-9] Round your answer to two places past the decimal. I can do basic pH questions but I am at a loss on this one. Please help.
Sunday, March 25, 2012 at 7:50pm by Brittany

Chemistry
You are treating this as an acid perhaps. NaOCl is a salt and the pH is determined by the hydrolysis of the salt; i.e., Kb of OCl^-. ........OCl^- + HOH ==> HOCl + OH^- I.......0.1M..............0.....0 C.......-x................x.....x E......0.1-x..............x.....x Kb ...
Monday, April 8, 2013 at 7:08pm by DrBob222

Chemistry
The base and acid are exactly neutralized; the pH is determined solely by the hydrolysis of the salt. (NH4Cl) = 50 mmols/200 mL = 0.25M. ......NH4^+ + H2O..> NH3 + H3O^+ I.....0.25.............0......0 C......-x..............x......x E.....0.25-x...........x......x Ka for ...
Thursday, May 2, 2013 at 5:46pm by DrBob222

chem.
a. the concentraion of Hion is 10^-6 pH then is defined as - log10 (10^-6)=6 b. find [H] from [H][OH]=10^-14 then conc H= 10^-14 / 10^-3 =10^-11 then find pH
Friday, December 18, 2009 at 12:40pm by bobpursley

chemistry
I assume these are two separate solutions; i.e., two separate problems. The pH of the NH4ClO4 solution is determined by the hydrolysis of the salt. NH4ClO4 is the salt of a weak base (NH3) and a strong acid (HClO4), therefore, the NH4^+ is hydrolyzed. NH4^+ + HOH ==> NH3 + ...
Saturday, April 18, 2009 at 3:05pm by DrBob222

chem
I didn't see that the pH at the equivalence point was in the question. I just looked again and it isn't. But the pH at the equivalence point is determined by the hydrolysis of the salt. Bu^- + HOH ==> HBu + OH^- Kb = (Kw/Ka) = (OH^-)(HBu)/(Bu^-) I think Kb is listed in the ...
Monday, March 1, 2010 at 11:38pm by DrBob222

chemistry
Run # Volume NaOH used (mL) 1 4.1 2 4.3 3 2.8 Concentraion of NaOH: 0.113 M pH of acid: 2.84 the questions are: #moles of NaOH: ? initial acid concentration: ? Determine the Ka and pka of the weak acid: ? So here is what I did: Shaked for several minutes about 1 g of the acid ...
Sunday, July 15, 2012 at 7:53pm by fenerbahce

Chem
HA(aq)+ H2O (l) <-> H3O+(aq)+ AŻ (aq) Given the reaction above, which of the following will cause an increase in the pH of an equilibrium mixture? Give all answers which apply. A) add KA B) add HA C) remove AŻ D) remove HA E) none of these will affect the pH.
Wednesday, February 9, 2011 at 9:35am by Michael

Chemistry
Solution A is 2.40M. 20mLs of solution A is transferred to a 250mL volumetric flask and diliuted to volume with water. What is the concentration of the diluted solution?
Thursday, April 25, 2013 at 6:10pm by Jaime

Chemistry
NH3 + HOH ==> NH4^+ + OH^- Write Kb expression. (NH4^+) = x molar (OH^-) = x molar (NH3) = (1 - x) molar Solve for x which = (OH^-) then pOH = - log(OH^-) and pH + pOH = pKw = 14 Solve for pH. Post your work if you need additional help.
Friday, November 23, 2007 at 9:15pm by DrBob222

Chem
The problem here, Lena, is that [pH][pOH]=1 x 10^-14 is not true. Two errors. pH + pOH = pKw = 14 which is the log form. If you wish to use the regular form it is or (H^+)(OH^-)=Kw = 1 x 10^-14 You mixed the two.
Monday, July 27, 2009 at 1:32am by DrGog222

chemistry
assume all of the ionized aspirin remains in the buffer solution and all of the un-ionized aspirin goes into to the ethyl acetate, what is the molarity of the aspirin in the ethyl acetate at pH 2 and pH 8? what equation would ou use for this?
Wednesday, April 3, 2013 at 8:31pm by kelly

biochemistry
if 4 volumes of 0.1M monobasic potassium phosphate, KH2PO4, are mixed with 2 volume of 0.1 M dibasic sodium phosphate, Na2HPO4, what will be the pH of the mixture? What if 4 volumes of 0.1 M KH2PO4 are mixed with 8 volumes of 0.1 M ethanolamine base(pka=9.44) what will be pH ...
Friday, January 21, 2011 at 7:32pm by dIrk

Chemistry
For the reaction of hydrazine (N2H4) in water, Kb is 3.0 10-6. H2NNH2(aq) + H2O(l)--> H2NNH3+(aq) + OH-(aq) Calculate the concentrations of all species and the pH of a 1.6 M solution of hydrazine in water. [OH-] = [H2NNH3+] = [H2NNH2] = [H+] = pH =
Sunday, February 3, 2013 at 4:26pm by Daniel

chem
DrBob has given you the equation to use: k2 = [H^+][SO4^-]/[HSO4^-] and the values to substitute [H^+] = 0.01 + x [SO4^-2] = x [HSO4^-] = 0.01 - x k2 = 1.2 x 10^-2 you need to substitute these and solve for x. Remember that you are after 0.01+x [H^+] to calculate the pH. is ...
Wednesday, March 26, 2008 at 12:42pm by lyne

chemistry lab titration
so for 0mL added would it be k3 = [(HAsO4^-2)(OH^-)/(AsO4^-)] K3 = (x^2)/(0.1M of AsO4) pk3 = -log k3. then solve for x which would give you [OH^-] which you could use to find pOH and find pH by using pH + pOH = pKw??
Wednesday, April 7, 2010 at 5:55pm by tara

chemistry
A 50.00ml sample of 0.200M hydroflouric acid (HF) is titrated with 0.200M NaOH. The Pka of HF is 3.452. a) calculate the pH of the HF solution before titration b) calculate the pH after the addition of 20.00ml of NaOH
Saturday, November 6, 2010 at 5:04pm by michelle

Chemistry
HC2H3O2 + NaOH --> NaC2H3O2 + H2O? a. when the titration is only half over, what species are present in the reaction flask b. what can be said about the pH at this point when the titration is half over? c. what is the pH at the equivalence point of this titration? 7, >7...
Monday, April 4, 2011 at 3:14pm by Anonymous

Chemistry
HCl is a strong acid. So is HBr. They ionize 100%. (H^+) from HCl = 0.035 moles/L. That from HBr is 0.080 moles/L. Add together to find total moles/L, then pH = -log(H^+). To find pOH, remember pH + pOH = pKw = 14.
Saturday, July 23, 2011 at 10:53pm by DrBob222

science
which has a lower ph pure water that is hot or pure water that is cold? is it possible for water to be neutralbut have a ph less than or greater than 7.0? how readily an acid donates a hydrogen is a fuction of how well the acid is able to accomodate the resulting negative ...
Friday, May 14, 2010 at 8:24pm by sarah

Chemistry
I don't get this at all. A beaker with 105mL of an acetic acid buffer with a pH of 5.00 is sitting on a bench top. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 8.40 mL of a 0.470 M HCl solution to the beaker. How much will the pH ...
Sunday, March 25, 2012 at 2:31pm by Amanda

Chemistry
The pH at the half-way point of a monoprotic acid is just pKa. For a monoprotic base (C2H5NH2) it is pKa but remember they give you pKb in the problem so pKa = 14-pKb. The pH at the equivalence point of a monoprotic acid or monoprotic base is calculated from the hydrolysis of ...
Friday, June 1, 2012 at 5:13pm by DrBob222

chemistry
A 0.5215 gram sample of CaCO3 is dissolved in 12M HCl and the resulting solution is diluted to 250.0 mL in a volumetric flask. How many moles of CaCO3 are used?
Tuesday, April 28, 2009 at 4:42pm by saddee

Chemistry
If gatorade has been diluted by a factor of 25 and reads 53.5 intensity units, what is the concentration of Na+ in the original gatorade? Is there a formula/equation use to solve for this?
Wednesday, August 11, 2010 at 12:26am by Anonymous

chem
How many grams of potassium permanganate (KMnO4) should be added to a 100 mL volumetric flask to prepare a 0.02505 M solution when the flask is diluted to the mark with water?
Wednesday, May 18, 2011 at 5:21pm by Amber

chemistry
How many grams of potassium hydrogen phthalate should be added to a 100 mL volumetric flask to prepare a 0.5000 M solution when the flask is diluted to the mark with water?
Thursday, May 19, 2011 at 12:31am by Shell

Chemistry
What will be the concentration if 52 milliters of a solution that is 12 parts per million in sodium chloride is diluted with enough water to make 97 millilters of solution?
Tuesday, February 14, 2012 at 1:36pm by Whitney

college chemistry
formt he diluted unknown concentration which i found to be 1.50mg/L i have to calculate the [Fe] in the PRIMARY unknown solution... that is placed in a 250mL volumetric flask
Wednesday, July 18, 2012 at 3:50pm by Anonymous

chemistry
a. molarity is defined as # moles/L solution. To find # moles, grams/molar mass. b. Look at the formula. There are two OH ions per Ba(OH)2 molecules; therefore, the concn of OH must be twice the answer to a. c. pOH = -log(OH). You have the OH from part b. d. pH + pOH = 14. You...
Tuesday, November 17, 2009 at 3:52pm by DrBob222

The first four are correct. lower pH is more acid. b. [H3O+]=log^-1 (9.5)=3.16E9 the antilog or log^-1 key might be the 10x key on your calculator. pOH=14-pH=14-9.5=4.5 [OH-]=antilog (4.5)=3.2E4 Notice [OH][H}= 1E14, which offers another way to solve it.
Tuesday, December 7, 2010 at 2:03pm by bobpursley

chemistry
Thymol blue in its acid range is not a suitable indicator for the titration of HCl by NaOH(aq) . Suppose that a student uses thymol blue by mistake in the titration of Figure 17-9 in the textbook and that the indicator end point is taken to be pH=2.0. Approximately what ...
Thursday, April 14, 2011 at 8:17am by sk1227

PH Calculation
Consider a 0.42 M solution of NaCH3COO CH3COO(aq) + H2O(l) -> CH3COOH(aq) + OH(aq) Calculate the pH of the solution at equilibrium. Try the weak acid or weak base approximation (as appropriate) and check the validity of the approximation. If the approximation is not valid...
Thursday, April 26, 2012 at 2:41am by RZeal

Chemistry
Question: Suppose you have 557 ml of 0.0300M HCL and you want to make up a solution of HCL that has a pH of 1.831. What is the maximum volume (in liters) that you can make of this solution? I know that you can get the concentration of HCL using the pH given, but how do you ...
Tuesday, March 3, 2009 at 10:05pm by eliz

chemistry
calculate the PH during the titration of 50.00 ml of 0.300 M HNO3 with 0.600 M KOH after 0, 15.50, 25.00, and 40.00 ml of KOH have been added. Graph the titration curve. Ph=
Friday, December 2, 2011 at 6:50pm by saud

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