Calculate the pH of a buffer system containing 0.25 M HF and 0.5 M NaF. (Ka for HF is 7.1 x 10-4)

What ratio of NaCN to HCN is needed to prepare a pH 10.10 buffer? (Ka of HCN is 4.9 × 1010)

What quantity in moles of HCl need to be added to 200.0 mL of a 0.200 M solution of NaF to make a buffer with a pH of 3.60? (Ka for HF is 6.8 × 10-4)

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 HCNO + 5.0 mL of 0.1 M NaOH   10 mL of 0.1 M HCNO + 10 mL of 0.1 M NaOH   10 mL of 0.1 M NH3 + 5.0 mL of 0.1 M HCl   10 mL of 0.1 M NH3 + 10 mL of 0.1 M HCNO

Suppose you have 500.0 mL of a buffer solution that made using 0.15 M of acid (HX) and the salt 0.13 M NaX. (Ka = 4.2 x 10-4) what is the pH of the buffer and net ionic equation.

Calculate the pH of a buffer that is 0.225 M HC2H3O2 and 0.162 M KC2H3O2, The Ka for HC2H302 is 1.8 x 10"

15.0 mL of a buffer is made by mixing 10.0 mL of 0.10 M HF and 5.0 mL of 0.10 M NaOH solution. What is the pH of this buffer after 0.24 mL of 1.0 M sodium hydroxide are added to it? The Ka for HF is 6.8 x 10-4.

How many moles of HCl need to be added to 200.0 mL of a 0.200 M solution of NaF to make a buffer with a pH of 2.80? (Ka for HF is 6.8 × 10⁻⁴)

How many grams of solid KF (molar mass = 58 g/mol) should be added to 1.00 L of 0.1 M HF to make a buffer of pH = 3.5? (Ka for HF = 7.20 X 10-4)

Calculate the molar ratio of NaFNaF to HFHF required to create a buffer with pH=4.20pH=4.20 . ( Ka(HF)=6.8×10−4Ka(HF)=6.8×10−4.)