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2 years ago

A. What is the pH of a solution with a [H+] of 6.8 x 10^-11?

Chemistry

1 answer:

inysia [295]2 years ago

6 0

Answer:

[H+] = 6.8×10^-11

so, pH = - log[H+]

= - log [6.8×10^-11]

= -(-10.167)

= 10.167

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$\displaystyle \frac{n({\rm CaCO_{3}})}{n({\rm CaCl_{2}})} = 1$ .

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$\begin{aligned} & n(\text{${\rm CaCO_{3}}$, theoretical}) \\ =\; & n({\rm CaCl_{2}}) \cdot \frac{n({\rm CaCO_{3}})}{n({\rm CaCl_{2}})} \\ \approx \; & 0.161023\; {\rm mol} \times 1 \\ =\; & 0.161023\; \rm mol\end{aligned}$ .

Calculate the theoretical yield of this experiment in terms of the mass of $\rm CaCO_{3}$ expected to be produced:

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3 years ago

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Learn more: brainly.com/question/22655760

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2 years ago