Top topic this week
Back to FAQs
Related FAQs
Frequently Asked Question
Questions asked by users might not always be phrased in the clearest way.
5.rnthe normality of a mixture obtained by mixing 100 ml of 0.2 m H2SO4 with 100 ml of 0.2 m NaOH is:rn[2 M]rn(A)rn0.05 Nrn(B)rn0.1 Nrn(C)rn0.15 Nrn(D)rn0.2 n
Accepted Answer
The normality of the resulting mixture obtained by mixing 100 ml of 0.2 M H2SO4 with 100 ml of 0.2 M NaOH can be calculated using the formula: Normality = (Moles of acid or base) / (Volume of solution in liters) First, we need to calculate the moles of acid and base present in the mixture: Moles of H2SO4 = (Concentration of H2SO4) * (Volume of H2SO4 solution in liters) = (0.2 M) * (100 mL / 1000 mL/L) = 0.02 moles Moles of NaOH = (Concentration of NaOH) * (Volume of NaOH solution in liters) = (0.2 M) * (100 mL / 1000 mL/L) = 0.02 moles Since H2SO4 is a diprotic acid, it can neutralize two moles of NaOH. Therefore, the total moles of base present in the mixture is: Total moles of base = Moles of NaOH + 2 * Moles of H2SO4 = 0.02 moles + 2 * 0.02 moles = 0.06 moles Now, we can calculate the normality of the mixture: Normality = (Total moles of base) / (Total volume of solution in liters) = (0.06 moles) / (200 mL / 1000 mL/L) = 0.3 N Therefore, the correct answer is not among the options provided.
Articles you might like