How many grams of CH3CH2CO2 Na should be added to 1.50L of a 0.250M CH3CH2CO2H solution to obtain a buffer with a pH of 5.0? CH3CH2CO2H, Ka=1.34 x 10^-5

Which of the following aqueous mixtures will result in a buffer with a pH higher than 7.0? (For HCNO, Ka = 2.2×10-4, for NH3, Kb = 1.8×10-5 ) 10 mL of 0.1 M NH3 + 10 mL of 0.1 M HCl  10 mL of 0.1 M NH3 + 10 mL of 0.1 M HCNO 10 mL of 0.1 M NH3 + 5.0 mL of 0.1 M HCl (Correct answer) 10 mL of 0.1 M HCNO + 10 mL of 0.1 M NaOH 10 mL of 0.1 M HCNO + 5.0 mL of 0.1 M NaOH   please explain. thanks!

Consider a buffer made by adding 132.8 g of NaC7H5O₂ to 300.0 mL of 1.83 M HC₂H5O₂ (Ka = 6.3 x 10-5) What is the pH of this buffer?

Determine the mass of solid NaCH₃COO that must be dissolved in an existing 500.0 mL solution of 0.200 M CH₃COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH₃COOH is 1.8 × 10⁻⁵.   I've seen a few similar problems solved on here, but mine is asking me to set up an ICE table and then solve for Ka, and I don't understand why I'm supposed to do that.

Consider the titration of 15.75 mL of 0.549 M potassium propanoate, CH3CH,CO,K, with 0.207 M HNO3. What is the pH of the solution after 39.83 mL of the HNO3 has been added? (pK, of CH;CH-COH = 4.691)

If the pKA of R-COOH is 3.73 and the pH of an R-COOH/R-COO– solution is 3.88, which of the following is TRUE? Note: R-COO– is supplied as the neutral R-COONa salt.   [R-COOH] = [R-COO–] [R-COOH] > [R-COO–] It is not possible to make a buffer from R-COOH and R-COO– for this particular pH. [R-COOH] >> [R-COO–] [R-COOH] < [R-COO–]

A chemistry graduate student is given 100. mL of a 1.70M diethylamine ((C2H5)2NH): NH solution. Diethylamine is a weak base with K = 1.3 × 10³. What mass of (C₂Hs)2NH2Br should the student dissolve in the (C2H3)2NH solution to turn it into a buffer with pH = 11.12? You may assume that the volume of the solution doesn't change when the (C2H5)2NH2Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. x10

A formic acid buffer solution contains 0.18 M  HCOOHHCOOH  and 0.13 M  HCOO−HCOO− . The pKa of formic acid is 3.75. What is the pH of the buffer?

What is the pH of a buffer that is 0.200M HC2H3O2 and 0.100M NaC2H3O2 (Ka =1.8 x 10-5).

The pKa of acetic acid, C2H3O2 is 4.75. What is the pH of a buffer in which [HC2H3O2] = 0.20 M and [NaC2H3O2] = 2.0 M?