8. b) Calculate the pH of a buffer that was prepared by mixing 45 mL of 0.01M aqueous hydrocyanic acid (HCN, Ka = 6.2 x 10-10) with 11 mL of 0.02M aqueous potassium hydroxide (KOH). %3D

Calculate the pH of a buffer solution that is 0.750 M CH3NH2 and 0.200 M CH3NH3Cl. For CH3NH2, Kb = 4.4*10-4

HA is a weak acid with a Ka  = 6.5 × 10-6 and a 45.0 mL sample of 0.10 M HA is titrated with 0.10 M NaOH. What is the pH after adding 20.0 mL NaOH?

An undergraduate research student wishes to create a system that mimics human blood (pH = 7.4). The student chose as the model system to use a buffer solution of sodium dihydrogen phosphate (NaH2PO4, Ka = 6.2 × 10–8) and sodium hydrogen phosphate (Na2HPO4, Ka = 4.2 × 10-13). A)  Which of the components of the buffer solution is the acid?  B)  Using the Henderson Hasselbalch equation, calculate the mole ratio of Na2HPO4/NaH2PO4 the student needs to use. C)  To approximate the human condition of blood alkalosis (where the pH of blood rises to 7.6, which is usually lethal), how much base will the student need to add to the buffer?

What is the pH of a 1.0 L buffer made with 0.300 mol of HF (Ka = 6.8 x 104) and 0.200 mol of NaF to which 0.050 mol of NaOH were added?

A buffer is formed by adding 1.0 mol of dimethylamine, (CH3)2NH, and 1.0 mol of dimethylammonium, (CH3)2NH2+, in a 1.0 L container. If a 10.0 mL sample of this buffer is diluted to 1000 mL with water, what is the pH of the diluted buffer?For dimethylamine, Kb = 5.4 × 10-4Insert your answer in decimal notation rounded to 2 decimal digits.

Consider a buffer made by adding 132.8 g of NaC₇H₅O₂ to 300.0 mL of 2.35 M HC₇H₅O₂ (Ka = 6.3 x 10⁻⁵) a What is the pH of this buffer?     b What is the pH of the buffer after 0.750 mol of H⁺ have been added?     c What is the pH of the buffer after 0.250 mol of OH⁻ have been added?

A buffer is prepared by mixing 25 mL of 0.10 M nitrous acid (HNO2) and 25 mL of 0.15 M sodium nitrite (NaNO2). The Ka for nitrous acid is 5.6 x 10-4. a.) What is the pH of the buffer solution? b.) What is the pH change when 5 mL of 0.10 M HCl is added to the solution?

Calculate pH of a buffer containing 0.10 M NH3 and 0.20 M NH4Cl. (Kb NH3 = 1.8 x 10-5).

To create a buffer solution, 40.00mL of a 0.100M benzoic acid (Bz) solution are mixed with 20.00mL of 0.100M sodium hydroxide solution. What is the pH of the resulting solution if the Ka of benzoic acid 6.5 x10 -5 and the pKa = 4.19? (Use the Henderson Hasselbach Equation with mmol). Reaction: HOBz + OH-  --->  H2O + OBz-   From the buffer solution above, youo take a 10.00mL portion of the buffer. Using all of the information provided, how much conjugate acid and conjugate base are in the 10.00mL portion that you took out? Group of answer choices 0.167mmol 0.500mmol 0.222mmol 0.333mmol