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A volume of $75 \mathrm{mL}$ of $0.060 \mathrm{M}$ NaF is mixed with $25 \mathrm{mL}$ of $0.15 \mathrm{M} \mathrm{Sr}\left(\mathrm{NO}_{3}\right)_{2} .$ Calculate the concentra-tions in the final solution of $\mathrm{NO}_{3}^{-}, \mathrm{Na}^{+}, \mathrm{Sr}^{2+},$ and $\mathrm{F}^{-} \cdot\left(K_{\mathrm{sp}} \text { for } \mathrm{SrF}_{2}=2.0 \times 10^{-10} .\right)$

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$$\begin{array}{l}{[N a+]=0.045 \mathrm{M}} \\{\left[N O_{3}^{-}\right]=0.075 \mathrm{M}} \\{\left[S r^{2+}\right]=0.015 \mathrm{M}} \\{\left[F^{-}\right]=1.15 \cdot 10^{-4} \mathrm{M}}\end{array}$$

Chemistry 102

Chapter 16

Acid-Base Equilibria and Solubility Equilibria

Acid-Base Equilibria

Aqueous Equilibria

University of Central Florida

University of Maryland - University College

Lectures

00:41

In chemistry, an ion is an atom or molecule that has a non-zero net electric charge. The name was coined by John Dalton for ions in 1808, and later expanded to include molecules in 1834.

24:14

In chemistry, a buffer is a solution that resists changes in pH. Buffers are used to maintain a stable pH in a solution. Buffers are solutions of a weak acid and its conjugate base or a weak base and its conjugate acid, usually in the form of a salt of the conjugate base or acid. Buffers have the property that a small change in the amount of strong acid or strong base added to them results in a much larger change in pH. The resistance of a buffer solution to pH change is due to the fact that the process of adding acid or base to the solution is slow compared to the rate at which the pH changes. In addition to this buffering action, the inclusion of the conjugate base or acid also slows the process of pH change by the mechanism of the Henderson–Hasselbalch equation. Buffers are most commonly found in aqueous solutions.

01:46

A volume of $75 \mathrm{~m…

09:38

A volume of 75 mL of 0.060…

06:34

A volume of $75 \mathrm{mL…

07:37

01:48

A chemist mixes equal volu…

01:51

$100.0 \mathrm{mL}$ of $1.…

01:58

A solution is prepared by …

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