If the pka of HCHO2 is 3.74 and the pH of an HCHO2/NaCHO2 solution is 3.89, which of the following is TRUE?
If the pka of HCHO2 is 3.74 and the pH of an HCHO2/NaCHO2 solution is 3.89
Question 2 2/2 pts If the pka of HCHO2 is 3.74 and the pH of an HCHO2/NaCHO2 solution is 3.89, which of the following is TRUE? It is not possible to make a buffer of this pH from HCHO2 and NaCHO2. [HCHO2] = [NaCHO2] [HCHO2] >>[NaCHO2] [HCHO2] < [NaCHO2] [HCHO2] > [NaCHO2] Question 3 1.33/2 pts Acid #1 has a pka of 3.15 Acid #2 has a pka of 3.65 Acid #3 has a pka of 4.23 Acid #4 has...
The best buffer system for maintaining a pH of 3.74 is: A. HCHO2/NaCHO2 B. HNO2 / NaNO2 C. HCN/NaCN Answer is A: How do you find this answer?
A buffer solution is to be formed using HCHO2 and NaCHO2. Ka for HCHO2 is 1.77 x 10-4. a. Find the mass of NaCHO2 that must be dissolved in 250. mL of 1.40 M of HCHO2 to prepare a buffer solution with pH = 3.36. b. What will be the pH of the solution following the addition of 15.0 mL of 0.0100 M NaOH?
compute the ph of reactants HCHO2 (.196M) and NaCHO2 (.271M) with a solution Ph of 4.4. Answer in 3 sig figs.
Part A a solution that is 0.20 M in HCHO2 and 0.15 M in NaCHO2 Part B a solution that is 0.11 M in NH3 and 0.22 M in NH4Cl
a 250.0 ml buffer solution initially contains 0.15 M HCHO2 and 0.10 M NaCHO2. what is the ph of this buffer? what component of the buffer must be added to change the ph to 3.91? what mass of this component must be added? assume negligible volume change
pKa value of formic acid is 3.74. calculate pH of a 0.25M solution of HCOONa the conjugate base of formic acid. Assume the coefficient are equal to 1?
Suppose a buffer solution is made from formic acid, HCHO2, and sodium formate, NaCHO2. What is the net ionic equation for the reaction that occurs when a small amount of sodium hydroxide is added to the buffer? Select one: a. H3O+(aq) + OH–(aq) → 2H2O(l) b. OH–(aq) + HCHO2(aq) → CHO2–(aq) + H2O(l) c. NaOH(aq) + H3O+(aq) → Na+(aq) + 2H2O(l) d. NaOH(aq) + HCHO2(aq) → NaCHO2(aq) + H2O(l)
ave the (4 pt) pKa 1.96 рКа 9,89 acid (HCHO2), pKa 3.74 5. Circle the strongest acid in each of the following groups (rows). (18 pt) a. H2S H20 H2Se НЕТе b. H20 HF CH4 NH3 C Hхо4 HXO2 нхоз HXO d. HAtO HCIO HIO HBro NH4 CsHsNH CoHsNH3 e. NHs, Ko 1.8x10- CSHSNH, K 1.7x10- CaHsNHa, K = 3.8 x 10-1 OH OH OH OH 6. Three oxoacids with the formular il strength:
Calculate the pH of the solution that results from each mixture. a. 50.0mL of 0.15M HCHO2 with 75.0mL of 0.13M NaCHO2 b.125.0mL of 0.10M NH3 with 250.0mL of 0.10M NH4CL