I need the steps to answer this question please! A buffer is prepared by adding 0.5...

Question

Question

I need the steps to answer this question please!

A buffer is prepared by adding 0.5 mol of solid sodium hydroxide to 1.0 L of 1.0 M acetic acid (CH3COOH). What is the pH of the buffer?

Answer 1

Answer #1

nNaOH = 0.5 mol (CH₂cool] =IM, I litr NCH₃Cool = (1x1) = Imol Pra (CH2COOH) = 4.744 - CHz Coona + H2O CH2 coole + NaOH os ini

Answer 2

Similar Homework Help Questions

Part A, B, C please Constants Periodic Tabl Part A A buffer is prepared by adding...

Part A, B, C please Constants Periodic Tabl Part A A buffer is prepared by adding 18.0 g of sodium acetate (CH3COONa) to 490 mL of a 0.145 M acetic acid (CH3COOH) solution. Determine the pH of the buffer. Express your answer using two decimal places. IVO AQ R O D ? pH = Submit Request Answer Part B Write the complete ionic equation for the reaction that occurs when a few drops of hydrochloric acid are added to the...
A buffer is prepared by adding 21.0 g of sodium acetate (CH3COONa) to 500 mL of...

A buffer is prepared by adding 21.0 g of sodium acetate (CH3COONa) to 500 mL of a 0.155 M acetic acid (CH3COOH) solution. Determine the pH of the buffer.
A buffer is prepared by adding 18.0 g of sodium acetate (CH3COONa) to 490 mL of...

A buffer is prepared by adding 18.0 g of sodium acetate (CH3COONa) to 490 mL of a 0.140 M acetic acid (CH3COOH) solution. 1) Determine the pH of the buffer. 2) Write the complete ionic equation for the reaction that occurs when a few drops of hydrochloric acid are added to the buffer. (Express your answer as a chemical equation. Identify all of the phases in your answer.) 3) Write the complete ionic equation for the reaction that occurs when...

What is the pH of a buffer prepared by adding 6.0 mol of acetic acid and...

What is the pH of a buffer prepared by adding 6.0 mol of acetic acid and 1 mol of NaOH to water to make a 1.0-L solution? Ka for acetic acid is 1.75*10-5 and its pKa is 4.76.
A buffer is prepared by adding 23.0 g of sodium acetate (CH3COONa) to 500 mL of...

A buffer is prepared by adding 23.0 g of sodium acetate (CH3COONa) to 500 mL of a 0.160 M acetic acid (CH3COOH) solution. Write the complete ionic equation for the reaction that occurs when a few drops of hydrochloric acid are added to the buffer. Write the complete ionic equation for the reaction that occurs when a few drops of sodium hydroxide solution are added to the buffer. Express your answer as a chemical equation. Identify all of the phases...
(1 point) A buffer solution is prepared by adding 20.0 mL of 0.100 M sodium hydroxide...

(1 point) A buffer solution is prepared by adding 20.0 mL of 0.100 M sodium hydroxide solution to 50.0 mL of 0.100 M acetic acid solution. What is the pH of the buffer?

A buffer is prepared by adding 20.0 g of sodium acetate (CH3COONa) to 480 mL of...

A buffer is prepared by adding 20.0 g of sodium acetate (CH3COONa) to 480 mL of a 0.160 M acetic acid(CH3COOH) solution. 1. Determine the pHpH of the buffer. 2. Write the complete ionic equation for the reaction that occurs when a few drops of hydrochloric acid are added to the buffer.Identify all of the phases in your answer. 3. Write the complete ionic equation for the reaction that occurs when a few drops of sodium hydroxide solution are added...
A buffer is prepared by adding 0.15 mol of lactic acid, CH3CHOHCOOH, and 0.20 mol of...

A buffer is prepared by adding 0.15 mol of lactic acid, CH3CHOHCOOH, and 0.20 mol of sodium lactate, Na+CH3CHOHCOO - , to sufficient water to make 1.0 L of buffer solution. The Ka of lactic acid is 1.4 x 10 - 4. Calculate the pH of the buffer.
A buffer solution was prepared by adding 4.72 g of sodium acetate, NaCH, CO2, to 2.50...

A buffer solution was prepared by adding 4.72 g of sodium acetate, NaCH, CO2, to 2.50 10 mL of 0.100 M acetic acid, CH3CO,H (K, = 1.8 x 10-6). a What is the pH of the buffer? pH = 5.10 Correct Find the pH using the Henderson-Hasselbalch equation: 4.72 g 1 mol NaCH, CO2 CH,CO2- ] = [NaCH,CO2] = 0.250 L -= 0.230 M 82.03 g [CH, CO2- pH = pK,+ logo = -log(1.8 x 10-5) + log CH, CO2H]...

a buffer solution of pH =5.30 can be prepared by dissolving acetic acid and sodium acetate...

a buffer solution of pH =5.30 can be prepared by dissolving acetic acid and sodium acetate in water. How many moles of sodium acetate must be added to 1 L of 0.25 M acetic acid to prepare the buffer? Ka(CH3COOH)=1.8 x 10^-5