A buffer solution contains 0.384 M KHCO3 and 0.239 M Na₂CO3. If 0.0464 moles of potassium hydroxide are added to 225.0 mL of this buffer, determine the pH of the resulting solution. Assume that the volume does not change upon adding potassium hydroxide. Given Ka of HCO3 = Ka2 of H₂CO3 = 4.7 x 10-11

A buffer solution is made that is 0.368 M in HCN and 0.368 M in KCN. If Ka for HCN is 4.00 × 10-¹0, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.088 mol HCl is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H3O+ instead of H+) + +

What is the pH of a solution that results when 3.00 mL of 0.034 M HCl is added to 0.200 L of a buffer solution is prepared from equal volumes of 0.200 M acetic acid and 0.600 M sodium acetate. (The Ka for acetic acid is 1.80 ×10-5.)

How many moles of hydrofluoric acid, HF, must be added to 150 mL of 0.31 M sodium fluoride to give a buffer of pH 3.25? Ignore the volume change due to the addition of hydrofluoric acid. ( Ka for HF is 6.8 x 10-4.)

The buffer was made by combining 0.220 M lactic acid (HC3H5O3) and 0.200 M sodium lactate ( NaC3H5O3). The Ka of HC3H5O3 is 1.4 x 10^-4. 1. write the equation describing the conjugate acid base relationship 2. Calculate the pH of the buffer 3. Calculate the pH of the buffer after the addition of 100.0 mL of 0.100 M potassium hydroxide to 0.9000 L of the buffer solution

45.0 mL of a buffer solution contains 0.20 M CH3COOH and 0.25 M CH3COONa. What is the pH of the mixture after 18.0 mL of 0.45 M HCI is added to this buffer solution? Ka of CH3COOH = 1.8 x 10-5.

A buffer solution is made that is 0.492 M in H2S and 0.492 M in KHS. If Ka1 for H2S is 1.00x10^-7, what is the pH of the buffer solution? pH =  Write the net ionic equation for the reaction that occurs when 0.135 mol NaOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.)   +       +

33. Consider a buffer solution that contains 0.45 M HCOOH and 0.55 M NaHCOO. Note that the Ka for formic acid (HCOOH) is 1.8 x 104. (a) Calculate the pH of this buffer solution. pH = (b) Write the net ionic chemical equation that occurs when potassium hydroxide (KOH) (MW of KOH = 56.1 g/mol) is added to the buffer. (c) If 0.260 g of solid KOH is added to 250. mL of this buffer solution, what is the resulting pH of the solution? New pH =

To simulate the pH of blood, which is 7.4, an undergraduate researcher in a biology lab produced a buffer solution by dissolving sodium dihydrogen phosphate (NaH2PO4, Ka = 6.2 × 10–8) and sodium hydrogen phosphate (Na2HPO4) together in an aqueous solution. What mole ratio of Na2HPO4/NaH2PO4 did she need to use?