Sunday
July 5, 2015

Search: Buffer solution ph

Number of results: 19,516

Chemistry
A 500.0-mL buffer solution is 0.100 M in HNO2 and 0.150 M in KNO2. Determine whether or not each of the following additions would exceed the capacity of the buffer to neutralize it. a. 250 mg NaOH b. 350 mg KOH c. 1.25 g HBr d. 1.35 g HI Can you explain to me how to go about ...
October 31, 2010 by Johannie

chemistry
2. A 350 mL buffer solution containing 0.15 M HF and 0.150 M NaF is reacted with sodium hydroxide. What mass of NaOH can this buffer neutralize before the pH rises above 4.0? If the same volume of buffer was 0.35 M in HF and 0.35 M in NaF then what mass of NaOH could be ...
December 1, 2010 by help

Chemistry
What is the Henderson-Hasselbach equation? Use the equation to determine the ratio of [A-] to [HA] necessary to create an ammonium chloride/ammonia buffer with a pH of 8.50. Describe how to make this buffer given a solution of 0.1 M NH3 (aq) and a bottle of NH4Cl(s).
March 4, 2012 by Lindsey

Biochemistry
A buffer is made at pH 7.3. 0.15 M using imidazole And 1 M hydrochloric acid to form the buffer. Can you show calculations for the formation of 500 mls of this buffer?
September 7, 2011 by Tommy

Chemistry
A solution is prepared by dissolving of pure HC2H3O2 and of NaC2H3O2 in of solution (the final volume). (a) What is the pH of the solution? (b) What would the pH of the solution be if of 0.250 M NaOH were added? (c) What would the pH be if of 0.40 M HCl were added to the ...
February 22, 2015 by Liam

chemistry
How would you go about increasing the buffering capacity of a phosphate buffer? I know that the answer is that you should increase the concentrations of the acid and base equally or increase the total volume of the buffer solution. But can someone explain why this works? Thanks.
January 30, 2012 by laura

Chemistry
1. Suppose that you have 0.500 L of each of the following solutions, and an unlimited supply of water. (Note: C9H7NHBr is a salt containing the ions C9H7NH+ and Br− and C9H7N is quinoline, an organic base with pKb = 6.24 at 298 K. If you like, you may represent C9H7NH+ ...
November 30, 2014 by Mcmaster university

chemistry
how do i know if the buffering capacity of a buffer solution is lost? Is that when after I add more of an acid or base to the solution that the pH eventually goes past + or - 1 of the original solution?
January 30, 2012 by laura

AP Chem
Calculate the correct volumes of the 0.1M acetic acid solution and the 0.1M sodium acetate solution needed to make 50mL of a buffer solution with a pH vaule of 5.00. (Ka = 1.8x10^-5)
March 11, 2012 by Keighley

Chmeistry
A lactic acid/lactate ion buffer solution contains 0.19 M HC3H5O3 and 0.78 M C3H5O3-, respectively. The Ka value of lactic acid is 1.4*10^-4. Calculate the pH of this buffer.
June 5, 2010 by Lynne

Chemistry
A lactic acid/lactate ion buffer solution contains 0.19 M HC3H5O3 and 0.78 M C3H5O3-, respectively. The Ka value of lactic acid is 1.4*10^-4. Calculate the pH of this buffer.
June 5, 2010 by Lynne

chemistry
A lactic acid/lactate ion buffer solution contains 0.43M HC3H5O3 and 0.90M C3H5O3-. The value of lactic acid is 1.4*10-4 calculate the pH of this buffer
June 16, 2015 by jennifer

chemistry 2
You are instructed to create 800. mL of a 0.69 M phosphate buffer with a pH of 7.6. You have phosphoric acid and the sodium salts NaH2PO4, Na2HPO4, and Na3PO4 available. what is the molarity needed for the acid component of the buffer?What is the molarity needed for the base ...
March 4, 2014 by Danielle

Chem 2
A popular buffer solution consist of carbonate (CO3 2-) and hydrogen carbonate (HCO3-) conjugate acid-base pair. Which, if any of the following such buffers has the highest buffer capacity? A. 0.9M CO3 2- and 0.1M HCO3- B. 0.1M CO3 2- and 0.9M HCO3- C. 0.5M CO3 2- and 0.5M ...
March 4, 2012 by Debbie

chemistry
calculate the change in pH when 9.00ml of 0.100M HCl(aq) is added to 100.0mL of a buffer solution that is 0.100M in NH3(aq) and 0.100M NH4Cl(aq). ...Calculate the change in pH when 9.00,L if 0.100M NaOH(aq) is added to the original buffer solution.
October 28, 2012 by mike

Chemistry
If you need to prepare 250.0 mL of a pH 5.00 buffer that has a total buffer concentration of acetic acid + sodium acetate of 0.050M, how many moles of each will you need to prepare the solution? Given solutions of acetic acid and sodium acetate with concentrations of 0.10M and...
November 11, 2013 by Natalie

chemistry
what is the pH of the buffer when 4ml of 1M HCl is added to a 100ml buffer solution made using 5ml 1M Na2HPO4 and 5ml 1M NaH2PO4? The pKa for H+ + HPO4- ==> H2PO4 is 6.82. What would happen to the pH if the 100ml buffer had been made up at the starting pH (6.82) using Tris...
August 23, 2010 by matt

chemistry
A 130.0 mL buffer solution is 0.100 M in NH3 amd 0.135 M in NH3 and 0.135 M in NH4Br. What mass of HCI could this buffer neutralize before the pH fell below 9.00?
November 6, 2011 by Samuel

chemistry
A reaction produced 0.40 mmol of H in a buffered solution which contained 300ml of 0.06M succinate buffer, pH is 4. What was the pH of the medium after the reaction was completed? The pKa of succinate buffer is 4.21
April 19, 2013 by veronica

Chemistry
I did an experiment on Buffers: In a polystyrene beaker, mix 20 ml of 0.1M Acetic acid ad 25 ml of 0.1 M sodium acetate and immediately measure the pH. Remove the electrode and add 5 ml of 0.1 M HCL to this buffer. Stir the solution and measure the pH. This is my data: Conc.of...
July 16, 2009 by Saira

chemistry
You have to prepare a pH 3.50 buffer and you have .10M HCOOH and .10M HCOONa, how many milliliters of each solution do you neeed for 1 liter of buffer
March 2, 2010 by Anonymous

Food Chemistry
Calculate the amounts and pH values for preparing the following acetic acid/acetate buffer solution. 1.) In the first step, If you plan to prepare a 2.00 M sodium acetate in 200.0 mL distilled water, how many grams of sodium acetate should be added in water? 2.) B. In the 2nd ...
April 29, 2010 by Lauren

CHEMISTRY
A buffer that is 0.271 M in acid, HA, and 0.150 M in the potassium salt of its conjugate base, KA, has a pH of 2.85. What is the pH of the buffer after 130. mL of 0.155 M LiOH is added to 0.650 L of this buffer? Assume that the volumes are additive.
September 21, 2011 by Rachel

CHEMISTRY
A buffer that is 0.271 M in acid, HA, and 0.150 M in the potassium salt of its conjugate base, KA, has a pH of 2.85. What is the pH of the buffer after 130. mL of 0.155 M LiOH is added to 0.650 L of this buffer? Assume that the volumes are additive.
September 21, 2011 by Rachel

chemistry
How many milliliters of a 0.250 M acetic acid solution must be added to 50.0 mL of a 0.750 M NaOH solution to produce a buffer solution with pH = 4.500 ? The pH is given by which we can calculate the concentration of [H+] How do we approach the problem from there?
April 22, 2015 by Anon

Chemistry
If a buffer solution is 0.190 M in a weak acid (Ka = 5.8 x 10^-5) and 0.550 M in its conjugate base, what is the pH? What if it said "if a buffer solution is ___ M in a weak base (Kb = ____) and ___ M in its conjugate acid, what is the pH? Would the steps from the first ...
April 22, 2012 by Katherine

chemistry
Write an equilibrium reaction for a buffer system made of the weak base, B, and its conjugate acid. If the buffer contains 1.05 M of B and 0.750M conjugate acid and has a pH of 9.50, what is the pH after 0.0050 mol HCl is added to 0.500 L of this solution?
April 9, 2012 by meme

Chemistry
a solution is made by combining 10.0 ml of 17.5 M acetic acid with 5.54 g of sodium acetate and diluting to a total volume of 1.50 L. a)calculate the pH of the solution. b) how many grams and milliliters of 14.6 M potassium hydroxide needs to be added so pH=pKa? c)what is the ...
November 29, 2011 by Amanda

Chemistry
A solution is prepared by dissolving 25.0 g of pure HC2H3O2 and 25.0 g of NaC2H3O2 in 700 mL of solution (the final volume). (a) What is the pH of the solution? (b) What would the pH of the solution be if 65.0 mL of 0.650 M NaOH were added? (c) What would the pH be if 40.0 mL ...
February 21, 2015 by Dean

Chemistry
You need to prepare 100.0 mL of a pH=4.00 buffer solution using 0.100 M benzoic acid (pKa = 4.20) and 0.220 M sodium benzoate. How much of each solution should be mixed to prepare this buffer? mL of benzoic acid ? mL of sodium benzoate?
March 27, 2015 by Ana

chemistry
a 350ml buffer solution is .150M in HF and .150M in NAF. What mass of naoh could this buffer neutralize before ph rises above 4.0? So far I got .285714 from 10^-.544. After that I tried to do .285714(x/.0525-x) but this doesn't worl. The answer is 1.2g. Help, please?
January 4, 2014 by Nancy

Chemistry(Please check, thank you)
For an experiment on the effect of a buffer solution, I need to calculate the expected pH of the buffer. I know that I have to make an amounts table and use the Hasselbalch equation to find the pH. For the first part, 0.10M HCl was added to a buffer. The first addition was 5 ...
March 29, 2012 by Hannah

chemistry
A buffer consists of 0.14 M KHCO3 and 0.61 M K2CO3. Carbonic acid is a dirpotic acid with Ka1= 4.5*10^-7 and Ka2= 4.7*10^-11. a) which Ka value is more important to this buffer b) what is the buffer pH?
March 7, 2013 by Justine

chemistry
What must be the minimum concentration of dichloroacetic acid in 1.00L buffer solution of a pH 0.91 dichloroacetic acid/sodium dichloroacetate buffer if the pH changes by 0.2 units when 0.057 moles HCl are added? Dichloroacetic Cl2CHCOOH ka= 5.50E-02 pka= 1.26
February 5, 2015 by Antonette

chemistry lab
Could someone help me with this? i am tired of it. here is my data from lab: Buffer1: HPO4- weight 3.412g; original pH Buffer 2: HEPES wt: 1.090g original pH 10.08 buffer1: pH of 0.1M: 7.5; pH of 0.01: 7.72; pH of 0.001M: 7.87 buffer2: PH of 0.1M: 7.5 ph of 0.01 M: 7.42 pH of ...
February 1, 2008 by amanda

Chemistry
You have 800 mL of a 0.050M phosphate buffer, pH 6.5. You need to increase the pH of this buffer to 7.5 by using 6.00M NaOH. Determine the volume of NaOH needed. What will be the final concentration of the buffer?
September 25, 2013 by Izabella

Chemistry. Help please
Calculate the pH of a buffer solution made by mixing 174 mL of a 1.68M trimethylamine (CH3)3N solution with 250 mL of a 1.08M trimethylammonia chloride, (CH3)3NHCl solution.
December 9, 2010 by Stephanie

chemistry
Calculate the change in pH when 6.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq). Calculate the change in pH when 6.00 mL of 0.100 M NaOH(aq) is added to the original buffer solution.
February 4, 2012 by Katie

chemistry
Calculate the change in pH when 6.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq). Calculate the change in pH when 6.00 mL of 0.100 M NaOH(aq) is added to the original buffer solution.
February 5, 2012 by Katie

CHEMISTRY
a) Calculate the change in pH when 4.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq). b) Calculate the change in pH when 4.00 mL of 0.100 M NaOH(aq) is added to the original buffer solution.
March 27, 2012 by Jematormal91

chemistry
Acetic acid (CH3COOH) has a Ka of 1.8x10^-5. a buffer is to be prepared with a pH of 5.00 from solutions of CH3COOH and sodium acetate (NaCH3COO) of the same concentration. How many mLs of NaCH3COO would have been added to 100 mL of CH3COOH to make the proper buffer solution??
November 19, 2013 by robyn

Chemistry
A buffer solution of pH=9.24 can be prepared by dissolving ammonia and ammonium chloride in water. How many moles of ammonium chloride must be added to 1.0 L of .50 M ammonia to prepare the buffer?
February 13, 2011 by Kate

Chemistry
How many grams of Na-benzoate (powder) do I need to prepare a buffer with pH = 4.2? How many grams of salt (NaCl) do I need to add to this buffer to make it a saturated solution of the salt? Thanks
June 23, 2011 by Ele

Chemistry
Calculate the pH of teh 0.20 M NH3/0.20 M NH4Cl buffer. What is teh pH of the buffer after the addition of 10.0 mL of 0.10 M HCl to 65.0 mL of the buffer?
May 11, 2011 by Kelly

Chemistry
True or False? A solution made from NaCl and HCl will act as a buffer solution.
June 2, 2010 by Heather

chemistry
As a technician in a large pharmaceutical research firm, you need to produce 200 mL of 1.00 M a phosphate buffer solution of pH = 7.06. The pKa of H_2PO_4}^- is 7.21. You have 2.00 L of 1.00 M KH_2PO_4 solution and 1.50 L of 1.00 M K_2HPO_4 solution, as well as a carboy of ...
May 11, 2012 by teja

chemistry
If 100 mL of .03 M HCL solution is added to 100 mL of buffer solution which is .1 M in NH3, and .1 M in NH4Cl, what will be the pH of the new solution?
November 13, 2010 by Audrey

chemistry
a 2.00l buffer contains 1.00 mol HNO3 mixed with 1.00mol NaNO2 a. write the relevant ionization equation for this buffer. b. determine its pH c. determine the new pH if 1.00g of NaOH is added to the buffer.
December 29, 2014 by mehek

chemistry
a 2.00l buffer contains 1.00 mol HNO3 mixed with 1.00mol NaNO2 a. write the relevant ionization equation for this buffer. b. determine its pH c. determine the new pH if 1.00g of NaOH is added to the buffer
January 1, 2015 by michelle

chemistry
If you mixed equal volume of .1 M HCl and .20 M Tris (pka=8.3), IS THE RESULTING SOLUTION A BUFFER SOLUTION? Why? or Why not?
September 18, 2010 by nicki

Biochemistry
what will be the pH of a buffer prepared by mixing 600 ml of 0.1M sodium acetate solution and 40 ml of 0.2M acetic acid solution
May 25, 2011 by Lisa

chemistry
12 mL of 0.0100 M HCl are added to 25.0 mL of a buffer solution that is 0.010 M HC2H3O2 and 0.08 M C2H3O2-. What is the pH of the resulting solution?
October 21, 2011 by tim

science
10 mL of 0.0100 M HCl are added to 25.0 mL of a buffer solution that is 0.010 M HC2H3O2 and 0.1 M C2H3O2-. What is the pH of the resulting solution?
March 15, 2013 by Erik

chemistry
10 mL of 0.0100 M HCl are added to 25.0 mL of a buffer solution that is 0.010 M HC2H3O2 and 0.1 M C2H3O2-. What is the pH of the resulting solution?
June 5, 2015 by Renata

chemistry
To 160.0 mL of a buffer solution containing 0.250 M ammonia and 0.100 M ammonium chloride, 20.00 mL of 1.00M HClO4 are added. a) Calculate the pH of the new solution. b) What becomes the pH if another 20.00 mL of the same acid solution is added?
February 15, 2013 by faizer

chemistry
As a technician in a large pharmaceutical research firm, you need to produce 200.mL of 1.00 M a phosphate buffer solution of pH = 7.19. The pKa of H2PO4− is 7.21. You have 2.00 L of 1.00 M KH2PO4 solution and 1.50 L of 1.00 M K2HPO4 solution, as well as a carboy of pure ...
September 14, 2013 by moses

Chemistry
As a technician in a large pharmaceutical research firm, you need to produce 100.mL of 1.00 M a phosphate buffer solution of pH = 7.45. The pKa of H2PO4− is 7.21. You have 2.00 L of 1.00 M KH2PO4 solution and 1.50 L of 1.00 M K2HPO4 solution, as well as a carboy of pure ...
March 31, 2014 by Billy Bob Reynolds

Chemistry
calculate the pH of a solution after .054 moles of KOH is added to a 1.0L buffer solution of .25M HF (Ka=7.1 x 10^-4) and .10M KF
April 24, 2014 by Aaron

Chemistry Homework Help
d 25 ml of 0.15 M HCL solution be added to 250 mL of buffer solution containing 0.25M HF Ka-7.1 x 10, and 0.40 M NaF at a pH of 3.15 what is the new pH?
November 24, 2014 by Always

Chemistry
Should 25 ml of 0.15 M HCL solution be added to 250 mL of buffer solution containing 0.25M HF Ka-7.1 x 10, and 0.40 M NaF at a pH of 3.15 what is the new pH?
November 24, 2014 by Always

Biochemistry
describe the preparation of 2litres of 0.2M acetate buffer of pH 5.5,starting from 2.5M solution of acetic acid and 2.5M solution of KOH{4.77}
April 19, 2015 by OCHAI

Chemistry
The of hydroxylamine, , is . A buffer solution is prepared by mixing 120 of a 0.34 hydroxylamine solution with 60 of a 0.25 solution.Solve for the PH
April 19, 2013 by Veronica

BioChem
Write the chemical equation for the reaction that occurs when you add NaOH solution to NaH2PO4/Na2HPO4 buffer solution
March 23, 2012 by Megan

Chemistry 1115
What is the chemical equation for the reaction that occurs when you add 0.1 M NaOH solution to the HC2H3O2-NaC2H3O2 buffer solution?
November 25, 2012 by Marci

chemistry8
1.why must MgCl2.6H20 be added to the EDTA solution? 2. why should EDTA solution be stored to the polyethylene container? 3. why should HCl be added to calcium carbonate solution? 4. why is it necessary to buffer the solution at pH 10 during titration?
July 17, 2010 by tan ni

Chem
calculate pH of the buffer solution prepared by mixing 10 mL of 1.5 M HCl with 100 mL of 0.1 M K2CO3 solution. For H2CO3: Ka1= 4.46 e^-7, Ka2= 4.69e^-11
November 12, 2008 by Sam

Please Help Me With This Chemistry HW Question!
Should 25 ml of 0.15 M HCL solution be added to 250 mL of buffer solution containing 0.25M HF Ka-7.1 x 10, and 0.40 M NaF at a pH of 3.15 what is the new pH?
November 25, 2014 by Always

Chemistry
What mass of solid sodium acetate, NaCH3COO, must be added to 2.50 L of an aqueous solution of 0.55 M acetic acid, CH3COOH, in order to make a buffer solution whose pH is 4.50? Assume that adding the solid does not change the volume of the solution.
December 15, 2012 by Dee

chemistry
Calculate the change in pH when 4.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq). Delta pH=? Calculate the change in pH when 4.00 mL of 0.100 M NaOH(aq) is added to the original buffer solution. Delta pH=?
July 8, 2012 by rachel

Chemistry
Consider the following buffer equilibrium: HF (high concentration) + H2O <--> H3O+ (low concentration) + F- ( high concentration) Using Le Chatelier's Principle, explain what happens to the pH of the buffer solution when a small amount of NaOH is added. Wouldn't OH- ...
June 3, 2010 by sh

ChemB
CALCULATE PH OF THE SOLUTION THAT RESULTS FROM EACH SOLUTION A) 150.0mL OF 0.25M HF WITH 225.0 mL OF 0.30M NaF Help please, these buffer questions are confusing.
March 12, 2012 by ALISON

Chemistry
You have 475 mL of an 0.47 M acetic acid solution. What volume (V) of 1.10 M NaOH solution must you add in order to prepare an acetate buffer of pH = 5.00?
January 19, 2013 by Mark

chemistry
A particular weak acid (HA) with a Ka of 2.0e-5 is 75% titrated with a strong base to produce a buffer solution. What is the pH of this final solution? Show all work.
March 24, 2015 by Nicole

Chemistry
A beaker with 150 mL 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 5.60 mL of a 0.280 M HCl solution to the beaker. How much will the pH change? The pKa of acetic ...
July 9, 2009 by Saira

chemistry help!!
A beaker with 195 mL 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 8.20 mL of a 0.260 it M HCl solution to the beaker. How much will the pH change? The pKa of acetic ...
July 13, 2009 by DrFunk

Chemistry
A beaker with 150 mL 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 7.90 mL of a 0.480 M HCl solution to the beaker. How much will the pH change? The pKa of acetic ...
October 6, 2009 by Anonymous

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 ...
July 22, 2013 by pablo

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...
January 11, 2009 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...
January 11, 2009 by Anonymous

Chemistry
Calculate the pH of a buffer solution made by mixing 231 mL of a 1.04M trimethylamine (CH3)3N solution with 176 mL of a 1.38M trimethylammonia chloride, (CH3)3NHCl solution. Enter your answer to TWO decimal places. DO NOT use scientific notation.
November 23, 2014 by Bill

CHEMISTRY
In a chemically active extraction, a three-component mixture of acetylsalicylic acid, acetaminophen, and caffeine in ethyl acetate solution is separated into its individual components first by extraction with a pH 8 buffer solution, then a subsequent extraction with dilute ...
September 9, 2012 by Gabby

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 ...
March 25, 2012 by Amanda

chemistry
A beaker with 1.40102mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 7.10mL of a 0.370M HCl solution to the beaker. How much will the pH change? The pKa of acetic ...
April 22, 2014 by Jennifer

Chemistry
A) Determine the pH of a 0.98 x 10^-2 mol L solution of hydrocyanic acid (HCN) Ka = 4.0 x 10^-10 B) What is the pH of a 0.243mol L solution of methylamine? (pKb for CH3NH2 = 3.30) C) determine the pH of a buffer solution of Na2CO3 (pkb = 3.68, 0.125 M) and NaHco3 (0.35M)
June 3, 2013 by Jake

Buffer Solutions
A buffered solution is made by adding 75.0g sodium acetate to 500.0 mL of a .64 M solution of acetic acid. What is the pH of the final solution? (Ka for acetic acid, CH3COOH, is 1.8 x 10^-5)
April 6, 2009 by Bob

Chemistry
A buffer solution is prepared by dissolving 0.400 mol of CH3COOH and 0.200 mol of CH3COONa in 1.00 L of water. 1.00 mL of 10.0 M HCl is added to a 100 mL portion of this solution. What is the final pH of the resulting solution? Ka of CH3COOH = 1.8 x 105
June 26, 2011 by Kendra

Chemistry
A buffer solution is prepared by dissolving 0.400 mol of CH3COOH and 0.200 mol of CH3COONa in 1.00 L of water. 1.00 mL of 10.0 M HCl is added to a 100 mL portion of this solution. What is the final pH of the resulting solution? Ka of CH3COOH = 1.8 x 105
June 26, 2011 by Sandy

Chemistry
How do the following solutions show the properties of a buffer? 1) 50 ml 0.10 M NH3 + 50 ml 0.10 M NH4NO3 2) 10 ml solution #1 + 5 ml H2O + 1 ml 0.10 M HCl 3) 10 ml solution #1 + 6 ml 0.10 M HCl 4) 10 ml solution #1 + 5 ml H2O + 1 ml 0.10 M NaOH
March 20, 2013 by Jeremy

chemistry (buffers)
How can weak acid nitrous acid HNO2 form a buffer solution with equal concentrations and volumes with weak base NH3? I thought that buffer solutions only occured between weak acids and strong bases or vice versa. The example above as two weak soltuions.
September 1, 2008 by mike

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 ...
November 12, 2012 by Bella

Biology
You have a stock solution with following components: glucose: 44 g/L NaCl: 191 g/L Tris Buffer: 275 g/L You mix 71 mL of the solution with water and bring the resulting solution to a final volume of 750 mL. What is the final concentration of glucose in g/L?
February 10, 2015 by Dee

CHEMISTRY
Suppose that you have 0.500 L of each of the following solutions, and an unlimited supply of water. (Note: C9H7NHBr is a salt containing the ions C9H7NH+ and Br- and C9H7N is quinoline, an organic base with pKb = 6.24 at 298 K. If you like, you may represent C9H7NH+ as HB+ and...
November 28, 2012 by sabrina: Please help

CHEMISTRY
Suppose that you have 0.500 L of each of the following solutions, and an unlimited supply of water. (Note: C9H7NHBr is a salt containing the ions C9H7NH+ and Br- and C9H7N is quinoline, an organic base with pKb = 6.24 at 298 K. If you like, you may represent C9H7NH+ as HB+ and...
November 28, 2012 by sabrina: Please help

chemistry
6.25 L of a propanoic acid-propanoate buffer must be prepared. The pH of the buffer needs to be 5.05. The solution will be 0.120M in propanoic acid. If the propanoate ion comes from the strontium propionate Sr(C3H5O2)2 then how many grams of strontium propanoate are needed?
March 1, 2013 by Studious

chemistry
Why is an Fe3+ solution instead of an Fe2+ solution used in calibrating the spectrophotometer? Note: hydroxylamine hydroxide is added to the Fe3+ solution then 1,10 phenanthroline is added to the solution after the addition of hydroxylamine hydroxide. After these additions, a ...
September 15, 2007 by smiley

Chemistry
1)A buffer solution that is 0.10 M sodium acetate and 0.20 M acetic acid is prepared. Calculate the initial pH of this solution. The Ka for CH3COOH is 1.8 x 10-5 M. As usual, report pH to 2 decimal places. *A buffered solution resists a change in pH.* 2)Calculate the pH when ...
March 10, 2015 by JUNDY

Chemistry
1)A buffer solution that is 0.10 M sodium acetate and 0.20 M acetic acid is prepared. Calculate the initial pH of this solution. The Ka for CH3COOH is 1.8 x 10-5 M. As usual, report pH to 2 decimal places. *A buffered solution resists a change in pH.* 2)Calculate the pH when ...
March 10, 2015 by JUNDY

Chemistry
Calculate the mass in g of aniline (C6H5NH2, Kb = 4.3 x 10-10) that must be added to 1.4 x 102 mL of 0.24 M (C6H5NH3)Cl solution in order to generate a buffer solution of pH 5.56. Give your answer to 2 significant figures. Noclue...
November 24, 2007 by Andrew

chemistry
An aqueous solution contains 0.445 M ethylamine (C2H5NH2). How many mL of 0.226 M hydrochloric acid would have to be added to 150 mL of this solution in order to prepare a buffer with a pH of 10.200
March 16, 2015 by chem

Chem II
Find the mass of sodium formate that must be dissolved in 200.00cm^3 of a 1.0M solution of formic acid to prepare a buffer solution with pH=3.40? I have no clue how to work this out. Please help me.
November 19, 2012 by Bianca

  1. Pages:
  2. <<Prev
  3. 1
  4. 2
  5. 3
  6. 4
  7. 5
  8. 6
  9. 7
  10. 8
  11. 9
  12. 10
  13. 11
  14. 12
  15. 13
  16. 14
  17. 15
  18. Next>>

Members