---### Titration Problem**Problem Statement:**20.0 mL of 1.0 M LiOH is added to 50.0 mL of 0.20 M H₂SO₄. What is the pH at this point in the titration?**Chemical Reaction:**\[ \text{H}_2\text{SO}_4 + 2\text{LiOH} \rightarrow \text{Li}_2\text{SO}_4 + 2\text{H}_2\text{O} \]**Question:** \[ \text{pH} = \text{[ ? ]} \]**Hint:** How many moles of H\(^+\) and OH\(^-\) are present? Consider the mole ratios.---### ExplanationTo determine the pH of the solution after the reaction, we need to follow these steps:1. **Calculate moles of H₂SO₄ and LiOH:** - Moles of H₂SO₄: \[ \text{Moles of H}_2\text{SO}_4 = M \times V = 0.20 \text{M} \times 50.0 \text{mL} \times \frac{1 \text{L}}{1000 \text{mL}} = 0.01 \text{moles} \] - Moles of LiOH: \[ \text{Moles of LiOH} = 1.0 \text{M} \times 20.0 \text{mL} \times \frac{1 \text{L}}{1000 \text{mL}} = 0.02 \text{moles} \]2. **Identify the limiting reagent:** - Given the balanced equation, 1 mole of H₂SO₄ reacts with 2 moles of LiOH. - The mole ratio of H₂SO₄ to LiOH is 1:2. 3. **Calculate the reaction completion:** - 0.01 moles of H₂SO₄ would require 0.02 moles of LiOH to completely react. - As there are exactly 0.02 moles of LiOH, both react completely.4. **Determine the final ionic concentrations:** - After reaction, none of

Given the volume of 1.0 M LiOH taken for titration = 20.0 mL Volume of 0.20 M H2SO4 taken for…

Answered: pH at this point in the titration?…

pH at this point in the titration? H₂SO4 + 2LIOH → Li₂SO4 + 2H₂O pH = [?] Hint: How many moles of H+ and OH- are present? Consider the mole ratios. pH at equivalence Enter

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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