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3 years ago

What kind of solvent(s) should be used to dilute magnesium nitrate and why?

Chemistry

1 answer:

son4ous [18]3 years ago

7 0

Answer:

Ethanol

Explanation:

As we know , magnesium nitrate is an ionic compound , because in water it easily dissociate into its corresponding ions , i.e. , Mg²⁺ and NO₃⁻ ions .

So , by using water as a solvent , will not work for Magnesium nitrate .

Hence ,

Ethanol can possibly be used as the solvent for the reaction of dilute magnesium nitrate , because , it is very less soluble in ethanol .

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3 years ago

Calculate the pKa of lactic acid (CH3CH(OH)COOH) given the following information. 3.005 grams of potassium lactate are added to

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Answer:

$\displaystyle \text{p} K_a \approx 3.856$

Explanation:

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$\displaystyle \begin{aligned} \left[ \text{KC$_3$H_$_5$O$_3$}\right] & = \frac{3.005\text{ g KC$_3$H_$_5$O$_3$}}{100.\text{ mL}} \cdot \frac{1\text{ mol KC$_3$H_$_5$O$_3$}}{128.17 \text{ g KC$_3$H_$_5$O$_3$}} \cdot \frac{1000\text{ mL}}{1\text{ L}} \\ \\ &= 0.234\text{ M}\end{aligned}$

By solubility rules, potassium is completely soluble, so the compound will dissociate completely into potassium and lactate ions. Therefore, [KC₃H₅O₃] = [C₃H₅O₃⁺]. Note that lactate is the conjugate base of lactic acid.

Recall the Henderson-Hasselbalch equation:

$\displaystyle \begin{aligned}\text{pH} = \text{p}K_a + \log \frac{\left[\text{Base}\right]}{\left[\text{Acid}\right]} \end{aligned}$

[Base] = 0.234 M and [Acid] = 0.500 M. We are given that the resulting pH is 3.526. Substitute and solve for p<em>Kₐ</em>:

$\displaystyle \begin{aligned} (3.526) & = \text{p}K_a + \log \frac{(0.234)}{(0.500)} \\ \\ 3.526 & = \text{p}K_a + (-0.330) \\ \\ \text{p}K_a & = 3.856\end{aligned}$

In conclusion, the p<em>Kₐ </em>value of lactic acid is about 3.856.

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1 year ago

Which functional group does the molecule below have?

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2 years ago