Determine each of the following for a 0.130 M HBr solution: a)Calculate the volume, in milliliters,...

Determine each of the following for a 0.130 M HBr solution:

a)Calculate the volume, in milliliters, of HBr solution required to neutralize 46.0 mL of a 0.350 M LiOH solution .

Acetic acid has a Ka of 1.8×10⁻⁵.

b)What is the pH of a buffer solution containing 0.10 M HC2H3O2 (acetic acid) and 0.12 M C2H3O2−?

Expert Solution

2) pKa= -log Ka = -log (1.8*10^-5) = 4.74

Use the Henderson - Hasselbalch equation:

pH = pKa + log ([CH3COO-] /[CH3COOH]

It contain 0.10 M CH3COOH and 0.12 M CH3COO–.

So [CH3COOH]=0.10 and [CH3COO–]=0.12

pH = 4.74 + log (0.12/0.10)

pH = 4.74 + log 1.2

pH = 4.74 + 0.0791

pH = 4.819

queen_honey_blossom answered 2 years ago

Calculate the volume, in milliliters, of a 0.216 M NaOH solution that will completely neutralize each...

Calculate the volume, in milliliters, of a 0.216 M NaOH solution that will completely neutralize each of the following: 1.) 3.71 mL of a 1.32 M HNO3 solution. 2.) 8.10 mL of a 0.800 M H3PO4 solution.

1. Calculate the volume in milliliters (mL) of a 6.00 M NaOH solution needed to make...

1. Calculate the volume in milliliters (mL) of a 6.00 M NaOH solution needed to make 5.00 x 102 mL of a 0.100 M NaOH solution. (Recall that M = molar = mol/L, and show all your work). 2. An approximately 0.1 M NaOH solution was standardized with KHP by titration to a phenolphthalein endpoint. From the following data, calculate the average molarity of the NaOH. The molar mass of KHP is 204.22 g/mol. Trial 1 Trial 2 Mass of...

Determine each of the following for a 0.170 M HBr solution: A.[H3O+] B.pH C.pOH D.Write the...

Determine each of the following for a 0.170 M HBr solution: A.[H3O+] B.pH C.pOH D.Write the balanced equation for the reaction with LiOH. E. Calculate the volume, in milliliters, of HBr solution required to neutralize 46.0 mL of a 0.160 M LiOH solution .

Determine the chloride ion concentration in each of the following solutions: 0.130 M BaCl2: M 0.666...

Determine the chloride ion concentration in each of the following solutions: 0.130 M BaCl2: M 0.666 M NaCl: M 1.802 M AlCl3: M (b) What is the concentration of a Sr(NO3)2 solution that is 1.55 M in nitrate ion? M

Calculate the pH of a 2.30×10-8 M solution of HBr.

calculate the pH of a 4.20x10^-8 M solution of HBr with water

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

A) A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH after the addition of 20.0 mL of KOH. B) 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 28.0 mL of HNO3. C) 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 15.0 mL of NaOH.

Question

Determine each of the following for a 0.130 M HBr solution: a)Calculate the volume, in milliliters,...

Solutions

Expert Solution

Related Solutions