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salantis [7]
3 years ago
5

The mass of a quantity of NiCl2

Chemistry
2 answers:
professor190 [17]3 years ago
8 0

<u>Answer:</u> The correct answer is Option A.

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

Given mass of nickel chloride = 24.6 g

Molar mass of nickel chloride = 129.6 g/mol

Putting values in above equation, we get:

\text{Moles of }NiCl_2=\frac{24.6g}{129.6g/mol}=0.19mol

Formula units is defined as lowest whole number ratio of ions in an ionic compound. It is calculate by multiplying the number of moles by Avogadro's number which is 6.022\times 10^{23}

We are given:

Number of moles of nickel chloride = 0.19 moles

Number of formula units = 0.19\times 6.022\times 10^{23}=1.1\times 10^{23}

Hence, the correct answer is Option A.

Gennadij [26K]3 years ago
3 0
Not sure, is it <span>:
</span>B.
<span> 1.9 3 1027 NiCl2
formula units</span>
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2H₂ + O₂ → H₂O

Explanation:

The unbalanced equation is

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In a balanced chemical equation, the number of moles of species on both sides of the expression must be the same.

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Number of moles          4           2                                   2           1

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8 0
3 years ago
Adding which of the following substances will decrease the solubility of calcium chloride in water: CaCl2(s) Ca2+(aq) + 2 Cl–(aq
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Answer:

Option b. Sodium chloride.

Explanation:

Consider the dissociation equilibrium of \rm CaCl_2 \; (s) in water:

\rm CaCl_2 \; (s) \rightleftharpoons Ca^{2+} \; (aq) + 2\; Cl^{-}\; (aq).

By the Le Chatelier's Principle, increasing the concentration of either product will shift the equilibrium to the left. Some \rm CaCl_2 \; (s) that was initially dissolved will precipitate out of the solution. This effect is called the common-ion effect.

For this \rm CaCl_2 \; (s) solution, the products of dissociation are

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Adding either to the solution will trigger the common-ion effect and reduce the solubility of \rm CaCl_2 \; (s).

In the two choices,

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  • Sodium fluoride \rm NaF will add \rm Na^{+} and \rm F^{-} ions to the solution.

\rm NaCl contains \rm Cl^{-} ions. It is capable of triggering the common-ion effect. However \rm NaF contains neither \rm Ca^{2+} ions nor \rm Cl^{-} ions. It will not trigger the common-ion effect.

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