What mass of HCl gas must be added to 1.00 L of a buffer solution that...

What mass of HCl gas must be added to 1.00 L of a buffer solution that contains [aceticacid]=2.0M and [acetate]=1.0M in order to produce a solution with pH = 3.73?

Solutions

Expert Solution

let molarity of HCl = x

[aceticacid]=2+x

[acetate]=1-x

PH = Pka + log[acetate]/ [aceticacid]

3.73 = 4.75 + log1-x/2+x

log1-x/2+x = 3.73-4.75

log1-x/2+x = -1.02

1-x/2+x = 10^-1.02

1-x/2+x = 0.0955

1-x = 0.0955*(2+x)

x = 0.74

molarity of HCl = x = 0.74 M

no of moles of HCl = molarity * volume In L

= 0.74*1 = 0.74 moles

mass of HCl = no of moles * gram molar mass

= 0.74*36.5 = 27.01g of HCl >>>>> answer

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

What amount of HCl gas must be added to 1.00L of a buffer solution that contains...

What amount of HCl gas must be added to 1.00L of a buffer solution that contains [aceticacid]=2.0M and [acetate]=1.0M in order to produce a solution with pH= 4.19?

Determine the pH change when 0.093 mol HCl is added to 1.00 L of a buffer...

Determine the pH change when 0.093 mol HCl is added to 1.00 L of a buffer solution that is 0.497 M in HNO2 and 0.311 M in NO2-. pH after addition − pH before addition = pH change = ___________________ Determine the pH change when 0.115 mol KOH is added to 1.00 L of a buffer solution that is 0.457 M in HNO2 and 0.256 M in NO2-. pH after addition − pH before addition = pH change =_____________

How much 10.0 M HNO3 must be added to 1.00 L of a buffer that is...

How much 10.0 M HNO3 must be added to 1.00 L of a buffer that is 0.0100 M acetic acid and 0.100 M sodium acetate to reduce the pH to 5.00? (pKa of acetic acid = 4.75)

0.2 mol of gaseous HCl is added to 1.0 L of a buffer solution that contains...

0.2 mol of gaseous HCl is added to 1.0 L of a buffer solution that contains 3.0 M CH3COOH and 3.0 M CH3COONa. What is the pH of the solution? Assume that Ka for CH3COOH is 10-5. Assume also that the volume of the solution does not change when the HCl is added. Type your answer in decimal number carrying only one digit after decimal. So you must round up or down at the second digit after decimal. For example,...

Calculate the pH if 0.03 mol HCl is added to 0.500 L of a buffer solution...

Calculate the pH if 0.03 mol HCl is added to 0.500 L of a buffer solution that is 0.24 M NH3 and 0.20 M NH4Cl? For NH3 Kb= 1.8 x 10-5

19.What quantity of NaOH(s) must be added to 1.00 L of 0.200 M HCl to achieve...

19.What quantity of NaOH(s) must be added to 1.00 L of 0.200 M HCl to achieve a pH of 12.00? (Assume no volume change.) 20.A 65.5-mL sample of 0.14 M HNO2 (Ka = 4.0 x 10–4) is titrated with 0.11 M NaOH. What is the pH after 26.8 mL of NaOH has been added? 21. What volume of 0.0100 M NaOH must be added to 1.00 L of 0.0500 M HOCl to achieve a pH of 8.00? Ka for HOCl...

1. What mass of sodium acetate, must be added to 1.00 L of 0.11 M acetic...

1. What mass of sodium acetate, must be added to 1.00 L of 0.11 M acetic acid to give solution with a pH of 4.40? Ka for acetic acid is 1.8*10^-5 2. When 700 mg of , lead fluoride, PBF2 is added to 1.00 L of water, the salt dissolves to a very small extent. At equilibrium, the concentration of Pb2+ is found to be 2.08*10^-3 M. What is the value Ksp of for PbF2?

Question