1) What volume of 0.25 M HNO3 (aq) reacts with 4.8 ml of 0.150 M Na2CO3 (aq) whe

Question

1) What volume of 0.25 M HNO3 (aq) reacts with 4.8 ml of 0.150 M Na2CO3 (aq) when the two solutions are mixed?please show work step by step.

2)A solution of hydrogen peroxide, H2O2, Is titrated with a solution of potassium permanganate, KMnO4. The reaction is

5H2O2(aq) + 2KMnO4 (aq) ?5O2 (g) + 2MnSO4 (aq) +K2SO4 (aq) + 8H2) (l)

It requires 51.7 mL of 0.145 M KMNO4 to titrate 20.0 grams of the solution of hydrogen peroxide. What it the mass percentage of H2O2 in the solution. Please show work step by step.

Explanation / Answer

molecular weight of H2O2=2+32=34

no .o fmoles of H2O2=20/34=0.588 moles

according to eqn 5 moles of H2O2 react with 2 moleds of KMnO4

so one mole of H2O2 ract with 2/5 moles of KMnO4

so 0.588 moles react with 0.588*(2/5)=0.2352 moles of KmnO4

weight of this no. of moles=0.2352*158=37.166

Total weight of solution=20+37.166=57.166

Weight % of H2O2=20/57.166 *100=34.98%

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