What is the pH made by combining 50.0 mL of 0.12 M HCN, 50.0 mL of 0.15 M NaCN and 2.0 mol NaOH?

What is the pH made by combining 50.0 mL of 0.12 M HCN, 50.0 mL of 0.15 M NaCN and 2.0 mol NaOH? Ka of HCN = 4.9 x 10^{-10} Assume the NaOH addition does not change the buffer volume.

Solutions

Expert Solution

This question is solved by using the simple concept of determination of pH of a solution having excess of moles in the solution.

The answer is given in the image,

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

What is the pH of a buffer made by combining 55.0 ml of 0.450 M HCN...

What is the pH of a buffer made by combining 55.0 ml of 0.450 M HCN and 45.0 ml of 0.250 M NaCN? (Ka of HCN = 4.4 x 10^-10) Use the Henderson Hasselbach equation, and prove why you can use it.

What is the pH of a solution obtained by adding 50.0 mL of 0.100 M NaOH...

What is the pH of a solution obtained by adding 50.0 mL of 0.100 M NaOH (aq) to 60.0 mL of 0.100 M HCl (aq)? Select one: a. 11.96 b. 2.04 c. 3.11 d. 7.00 QUESTION 2 What is the pH of a solution prepared by dissolving 5.86 grams of propanoic acid, CH3CH2COOH (l), and 1.37 grams of NaOH (s) in enough water to make exactly 250.0 mL of solution. pKa = 4.87 for propanoic acid? Select one: a. 4.58...

You are asked to prepare 2.0 L of a HCN/NaCN buffer that has a pH of...

You are asked to prepare 2.0 L of a HCN/NaCN buffer that has a pH of 9.6 and an osmotic pressure of 1.29 atm at 298 K. a) What mass of HCN should you use to prepare the buffer? b) What mass of NaCN should you use to prepare the buffer? (Assume complete dissociation of NaCN.)

A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH...

A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH after the addition of 13.0 mL of KOH. Express your answer numerically. A 75.0-mL volume of 0.200 M NH3 (Kb=1.8×10−5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 15.0 mL of HNO3. Express your answer numerically. A 52.0-mL volume of 0.35 M CH3COOH (Ka=1.8×10−5) is titrated with 0.40 M NaOH. Calculate the pH after the addition of 33.0 mL...

A buffer is made by adding 0.12 mol NH4Cl and 0.15 mol NH3 to enough water...

A buffer is made by adding 0.12 mol NH4Cl and 0.15 mol NH3 to enough water to make 0.250 L of solution. (Ka NH4+/NH3= 5.6 x10−10) a) Calculate the pH of the buffer solution b) What is the pH after the addition of 10.00 mL of 0.1 M NaOH to 90.00 mL of this buffer solution? Compare to pH in part a. c) What is the pH of a solution made by adding 10.00 mL of 0.1 M NaOH to...

What is the pH of a solution made by mixing 500 mL of 1.00 M HCN...

What is the pH of a solution made by mixing 500 mL of 1.00 M HCN and 1.50 L of 0.250 M NaOH, and then diluting the entire solution to a volume of 3.00 L? (Ka HCN = 4.0 x 10-10) A. 8.92 B. 6.52 C. 9.88 D. 9.27 E. 5.08 To obtain one litre of a solution of pH = 7, you should dissolve in water A. Two mol of HI + two mol of CH3NH2 B. One mol...

Calculate the pH during the titration of 50.0 mL of 0.116 M NaOH with 0.0750 M...

Calculate the pH during the titration of 50.0 mL of 0.116 M NaOH with 0.0750 M HNO3 at:a) 0 mL titrant b) 3 mL before equivalence c) at equivalence d) 3 mL past equivalence

Calculate the pH during titration of 25 mL of 0.175 M HCN with 0.3 M NaOH...

Calculate the pH during titration of 25 mL of 0.175 M HCN with 0.3 M NaOH after the addition of 0 mL, 7.29mL, 14.5833 mL, and 20 mL base. Show all work.

Calculate the pH during titration of 25 mL of 0.175 M HCN with 0.3 M NaOH...

Calculate the pH during titration of 25 mL of 0.175 M HCN with 0.3 M NaOH after the addition of 0 mL, 7.29mL, 14.5833 mL, and 20 mL base. Kb of CN- is 2.03 x 10^-5. Show all work.

50.0 mL of 2.00 mol/L HNO3 solution and 50.0 mL of 1.00 mol/L NaOH solution, both...

50.0 mL of 2.00 mol/L HNO3 solution and 50.0 mL of 1.00 mol/L NaOH solution, both at 20.0 degree Celsius, were mixed in a calorimeter. Calculate the molar heat of neutralization of HNO3 in kJ/mol if: (1) final temperature was 28.9 degree Celsius; (2) the mass of the overall solution was 102.0 g; (3) the heat capacity of the calorimeter was 25.0 J/C; (4) and assume that the specific heat of solution is the same as water, 4.184 J/(g C);

Subjects