What is the concentration of hydroxide ions after 50.0 mL of 0.250 M NaOH is added...

What is the concentration of hydroxide ions after 50.0 mL of 0.250 M NaOH is added to 120 mL of 0.200 M Na2SO4?

What is the concentration of hydroxide ions after 50.0 mL of 0.250 M NaOH is added to 120 mL of 0.200 M Sr(OH)2?

Solutions

Expert Solution

a) The moles of hydroxide ions added = Molarity of OH- X volume of OH- in litres = 0.250 X 50 X 10^-3 = 12.5 millimoles

The volume of solution = volume of OH- + volume of Na2SO4 = 50 + 120 = 170 mL

Now the new concentration of hydroxide ions = Initial moles of OH- / total volume

Concentration of hydroxide ions = 12.5 / 170 = 0.0735 Molar

b) The moles of hydroxide ions added = Molarity of OH- X volume of OH- in litres = 0.250 X 50 X 10^-3 = 12.5 millimoles

The moles of Sr(OH)2 added = Molarity of Sr(OH)2X volume of Sr(OH)2 in litres = 120 X 0.2 = 24 millimoles

Sr(OH)2 is a strong acid and will dissociates completely

1 mole of Sr(OH)2 will give two moles of Hydroxide ions

so 24 millimoles of Sr(OH)2 will give = 48 millimoles of OH-

total moles of OH- = 12.5 + 48 = 60.5 millimoles

total volume of solution = 120 + 50 = 170 mL

concentration of hydroxide ions = Moles / volume = 60.5 / 170 = 0.356 Molar

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

When 50.0 mL of 0.45 M HCl was added to 50.0 mL of 0.65 M NaOH,...

When 50.0 mL of 0.45 M HCl was added to 50.0 mL of 0.65 M NaOH, the temperature change was 5.8 *C. Calculate the heat change for the reaction (Qsoln) and the heat of neutralization (ChangeHneut), and the state whether the reaction is exothermic or endothermic.

When 50.0 mL of 0.45 M HCl was added to 50.0 mL of 0.65 M NaOH,...

500.0 mL of 0.140 M NaOH is added to 565 mL of 0.250 M weak acid...

500.0 mL of 0.140 M NaOH is added to 565 mL of 0.250 M weak acid (Ka = 8.39 × 10-5). What is the pH of the resulting buffer? HA(aq)+OH^-(aq)=H2O(l)+ A^-(aq) pH=?

A student added 50.0 mL of an NaOH solution to 100.0 mL of 0.300 M HCl....

A student added 50.0 mL of an NaOH solution to 100.0 mL of 0.300 M HCl. The solution was then treated with an excess of aqueous chromium(III) nitrate, resulting in formation of 2.36 g of precipitate. Determine the concentration of the solution.

50.0 ml of an acetic acid (CH3COOH) of unknown concentration is titrated with 0.100 M NaOH....

50.0 ml of an acetic acid (CH3COOH) of unknown concentration is titrated with 0.100 M NaOH. After 10.0 mL of the base solution has been added, the pH in the titration flask is 5.30. What was the concentration of the original acetic acid solution? (Ka(CH3COOH) = 1.8 x 10-5)

50.0 mL of 10.0 M sodium hydroxide is added to a 1.00 L solution containing 0.100...

50.0 mL of 10.0 M sodium hydroxide is added to a 1.00 L solution containing 0.100 M nickel (II) nitrate, 0.100 M tin (II) nitrate, and 0.100 M zinc nitrate. How many grams of tin (II) hydroxide precipitates from solution.

A 50.0 mL sample of 0.0645 M AgNO3(aq) is added to 50.0 mL of 0.100 M...

A 50.0 mL sample of 0.0645 M AgNO3(aq) is added to 50.0 mL of 0.100 M NaIO3(aq). Calculate the [Ag+] at equilibrium in the resulting solution. The Ksp value for AgIO3(s) is 3.17 × 10-8. [Ag+] =____ mol/L

Calculate the pH after 10 mL of 1.0 M sodium hydroxide is added to 60 mL...

Calculate the pH after 10 mL of 1.0 M sodium hydroxide is added to 60 mL of 0.5 M acetic acid.

What is the concentration of hydronium ions after a 100mL solution of 0.02M Magnesium Hydroxide and...

What is the concentration of hydronium ions after a 100mL solution of 0.02M Magnesium Hydroxide and 100mL of 0.05M nitric acid?

In a constant‑pressure calorimeter, 50.0 mL 50.0 mL of 0.800 M H2SO40.800 M H2SO4 was added...

In a constant‑pressure calorimeter, 50.0 mL 50.0 mL of 0.800 M H2SO40.800 M H2SO4 was added to 50.0 mL50.0 mL of 0.370 M NaOH.0.370 M NaOH. The reaction caused the temperature of the solution to rise from 23.40 ∘C23.40 ∘C to 25.92 ∘C.25.92 ∘C. If the solution has the same density and specific heat as water (1.00 g/mL1.00 g/mL and 4.184 J/(g⋅°C),4.184 J/(g⋅°C), respectively), what is Δ?ΔH for this reaction (per mole of H2OH2O produced)? Assume that the total volume...

Subjects