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leva [86]
3 years ago
13

1) When chromium chloride, CrCl2, is dissolved in water, the temperature of the water decreases. a) Is the heat of solution exot

hermic or endothermic? b) Which is stronger—the attractive forces between water molecules and chromium and chloride ions, or the combined ionic bond strength of CrCl2 and intermolecular forces between water molecules? Explain.
Chemistry
1 answer:
Mandarinka [93]3 years ago
3 0

Answer:

Explanation:  It has been given that the temperature of the water decreases when chromium chloride is dissolved in water. Thus fall in the temperature explains the fact that the bond energies of the reactants have more energy rather than the products.

a) Thus the heat of the solution is endothermic in nature as more energy is needed to break the reactant molecules.

b) The combined ionic bond strength of CrCl2 and inter molecular forces between water molecules must be stronger than the attractive forces between the  water molecules and chromium and chloride ions as the reaction is endothermic in nature thus more energy would be required to break the bonds between the reactants hence making them more stronger.

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Answer:

C

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Why does surface area of a reactant influence the rate of the reaction?
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Water boils at 100°C at sea level. If the water in this experiment did not boil at 100°C, what could be the reason?
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IgorC [24]

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Pyridinium is a weak acid having a pKa of 5.2. How much pyridine (the conjugate base of pyridinium) must be added to an aqueous
Whitepunk [10]

Answer:

Amount of pyridine required = 0.0316 M

Explanation:

pH of a buffer solution is calculated by using Henderson - Hasselbalch equation.

pH=pK_a+log\frac{[Conjugate\ base]}{[weak\ acid]}

Pyridinium is a weak acid and in the presence of its conjugate base, it acts as buffer.

Henderson - Hasselbalch equation for pyridine/pyridinium buffer is as follows:

pH=pK_a+log\frac{[Py]}{PyH^+]}

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PyH^+ (Pyridinium)=0.100 M

Substitute the values in the formula

pH=pK_a+log\frac{[Py]}{PyH^+]}\\4.7=5.2 log\frac{[Py]}{0.100}

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\frac{[Py]}{0.100} =0.316

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