General Chemistry
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Determine the pH for the following solution: 25.0 mL 0.17 M HIO with 35.0 mL 0.19 M NaIO (Ka HIO = 2.3×10−11)
Identify whether to add KOH or HBr to the buffer mixture to adjust the pH to 9.56. The buffer solution of 1-L initially contains 0.500 M in CH3NH2 and 0.500 M in CH3NH3Br. Calculate the mass of the correct reagent needed.
A buffer solution is prepared using HF and F–. HF has a pKa of 3.16 and the buffer has a pH of 3.35. Determine which of the following is applicable at pH 3.35 without performing any calculations.
Acetic acid is a weak acid that dissociates into acetate ion and hydronium ions in solutions:
CH3COOH(aq) + H2O(l) ⇌ H3O+(aq) + CH3COO-(aq)
The value of the dissociation constant (Ka) for acetic acid is 1.78×10-5. If you require a buffer of pH 5.25, what would be the ratio of [CH3COO-]/[CH3COOH] that you would use?
If you need to prepare a buffer with a pH of 8.8, which one of the following acid/conjugate base pairs would you choose?
Consider a 250.0 mL solution of 0.20 M propanoic acid. Calculate the mass of sodium propanoate needed to produce a buffer with a pH of 5.11 assuming the volume does not change.
Calculate the pH of the solution that results from each mixture. a. 50.0 mL of 0.15 M HCHO2 with 75.0 mL of 0.13 M NaCHO2
Consider a solution that contains 25 g of CH3COOH and 15 g of NaCH3COO in a 250.0 mL of solution
Calculate the pH using the Henderson–Hasselbalch equation.
Use the Henderson–Hasselbalch equation to calculate the pH of each solution.
c. a solution that contains 10.0 g of HC2H3O2 and 10.0 g of NaC2H3O2 in 150.0 mL of solution
A buffer contains a weak acid, HA, and its conjugate base. The weak acid has a pKa of 5.7, and the buffer has a pH of 5.2. Without doing a calculation, choose which of these possibilities is correct at pH 5.2.