Textbook Question
If 123 mL of a 1.1 M glucose solution is diluted to 500.0 mL, what is the molarity of the diluted solution?
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Ch.4 - Chemical Quantities & Aqueous Reactions
Chapter 4, Problem 65
Consider the precipitation reaction: 2 Na3PO4(aq) + 3 CuCl2(aq) → Cu3(PO4)2(s) + 6 NaCl(aq). What volume of 0.175 M Na3PO4 solution is necessary to completely react with 95.4 mL of 0.102 M CuCl2?
Verified step by step guidance1
Identify the balanced chemical equation: \(2 \text{Na}_3\text{PO}_4(aq) + 3 \text{CuCl}_2(aq) \rightarrow \text{Cu}_3(\text{PO}_4)_2(s) + 6 \text{NaCl}(aq)\).
Determine the moles of \(\text{CuCl}_2\) using its concentration and volume: \(\text{moles of } \text{CuCl}_2 = 0.102 \text{ M} \times 0.0954 \text{ L}\).
Use the stoichiometry of the reaction to find the moles of \(\text{Na}_3\text{PO}_4\) needed. According to the balanced equation, 2 moles of \(\text{Na}_3\text{PO}_4\) react with 3 moles of \(\text{CuCl}_2\).
Calculate the moles of \(\text{Na}_3\text{PO}_4\) required using the ratio from the balanced equation: \(\text{moles of } \text{Na}_3\text{PO}_4 = \frac{2}{3} \times \text{moles of } \text{CuCl}_2\).
Determine the volume of \(0.175 \text{ M } \text{Na}_3\text{PO}_4\) solution needed using its concentration: \(\text{Volume} = \frac{\text{moles of } \text{Na}_3\text{PO}_4}{0.175 \text{ M}}\).
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