A buffer solution is prepared by dissolving 1.000 g of sodium acetate (CH3COONa) into 100.00 mL of a 0.100 M solution of acetic acid. Then 3.00 mL of a 2.00 M solution of sodium hydroxide is added to the acetic acid/sodium acetate buffer solution. The Ka of acetic acid is 1.8 × 10−5.   What is the pH of the solution after adding NaOH?

The pH of a bicarbonate-carbonic acid buffer is 5.41. Calculate the ratio of the concentration of carbonic acid (H2CO3)to that of the bicarbonate ion (HCO3−).(Ka1 of carbonic acid is 4.2 ×10−7.)   [H2CO3]   [HCO3−] =

A buffer solution is 0.341 M in CH3COOH and 0.270 M in CH3COONa. If Ka for CH3COOH  is 1.8x 10^-5  , what is the pH of this buffer solution? pH =

Adding as little as 0.1 mL of concentrated HCl to a liter of H2O shifts the pH from 7.0 to 3.0. Adding the same amount of HCl to a liter of a solution that 0.1 M in acetic acid and 0.1 M in sodium acetate, however, results in a negligible change in pH. Why do these two solutions respond so differently to the addition of HCl?

A buffer solution is made that is 0.409 M H2S and 0.409 M in NaHS. 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 0.087 mol NaOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.)

A buffer solution is 0.405 M in H2CO3 and 0.397 M in KHCO3. If Kal for H2CO3 is 4.2 × 107, what is the pH of this buffer solution? pH =

2. If you make a solution by mixing 25.mL of 0.50 M acetic acid (CH3COOH) and 25 mL of 0.30 M sodium acetate (CH3COONa) together in a beaker: a. The Ka of acetic acid is 1.8 x 105. What is the pH of the solution that you made? What is the degree of ionization? CH&COOH+ CHeCOONat lOH 4 g CH300H

A buffer solution is formed by adding 0.200 moles of solid potassium nitrite, KNO₂, to 500.0 ml of 0.600 M Nitrous acid, HNO₂ solution. You may assume that the change in volume is negligible upon addition of the solid. Calculate the pH of the buffer solution Calculate the pH of the buffer solution after the addition of 8.00 ml of 1.50 M Ba(OH)₂.

An analytical chemist is titrating 169.4 mL of a 1.000M solution of butanoic acid (HC3H,CO₂) with a 1.100M solution of KOH. The pK of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 183.1 mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places. pH = ☑

Calculate the pH of a solution formed by adding 2.00 grams of solid potassium cyanide, KCN, to 180.0 ml of 0.340 M hydrocyanic acid solution, HCN. You may assume that the salt dissolves completely and that the change in volume is negligible upon addition of the solid.