Calculate the concentration (M) of copper in each sample. The Cu^2 standard solution was prepared...
Question:
Calculate the concentration (M) of copper in each sample. The {eq}\displaystyle \rm Cu^2 {/eq} standard solution was prepared by dissolving {eq}\displaystyle \rm 3.928 \ g \ CuSO_4 \cdot 5H_2O {/eq} into {eq}\displaystyle \rm 1.000 \ L {/eq} distilled water.
The {eq}\displaystyle \rm NH_4OH {/eq} used in these solutions is {eq}\displaystyle \rm 3 \ M {/eq}. Following are the mixtures for the solutions:
Solution {eq}\displaystyle \rm 1: 7.50 \ mL {/eq} standard {eq}\displaystyle \rm Cu^{2+}: 0.00 \ mL, \ H_2O: 2.50 \ mL \ NH_4OH {/eq}
Solution {eq}\displaystyle \rm 2: 6.00 \ mL {/eq} standard {eq}\displaystyle \rm Cu^{2+}: 1.50 \ mL \ H_2O: \ 2.50 \ mL \ NH_4O {/eq}
Volume:
Volume is one factor on which the molarity of a solution depends. If the volume of a solution is either increased/decreased by adding/removing the solvent, then the molarity of a solution changes.
Answer and Explanation: 1
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View this answerThe amount of {eq}\rm CuSO_4.5H_2O {/eq} in its standard solution is 3.928 g.
The molar mass of {eq}\rm CuSO_4.5H_2O {/eq} is 159.6 g/mol
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Chapter 9 / Lesson 2Learn about the mole ratio. Understand the definition of mole ratio, how to find mole ratio in stoichiometry, and see examples of using mole ratio in problems.
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