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4 years ago

Given the following balanced chemical equation:

Chemistry

1 answer:

Fudgin [204]4 years ago

7 0

Answer:

Mass of Ca(OH)₂ required = 0.09 g

Explanation:

Given data:

Volume of HNO₃ = 25 mL (25/1000 = 0.025 L)

Molarity of HNO₃ = 0.100 M

Mass of Ca(OH)₂ required = ?

Solution:

Chemical equation;

Ca(OH)₂ + 2HNO₃ → Ca(NO)₃ + 2H₂O

Number of moles of HNO₃:

Molarity = number of moles / volume in L

0.100 M = number of moles / 0.025 L

Number of moles = 0.100 M ×0.025 L

Number of moles = 0.0025 mol

Now we will compare the moles of Ca(OH)₂ with HNO₃ from balance chemical equation.

HNO₃ : Ca(OH)₂

2 : 1

0.0025 : 1/2×0.0025 = 0.00125

Mass of Ca(OH)₂:

Mass = number of moles × molar mass

Mass = 0.00125 mol × 74.1 g/mol

Mass = 0.09 g

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$pH = -Log ([H^{+}]) = 1$

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(a) and (c) are strong acids so they dissociate completely in aqueous solution. Thus, the concentration of the acid is the same as the protons.

(b) and (e) are strong bases so they dissociate completely in aqueous solution too. Thus, the concentration of the base is the same as the oxydriles. But in this case it is necessary to consider the water autoionization to calculate the protons concentration:

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clearing the $[H^{+} ]$

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(d) is a weak base so it is necessary to solve the equilibrium first, knowing $Ka=3.24x10^{-8}$

The reaction is $HClO$ → $H^{+} + CO^{-}$ so the equilibrium is

$Ka=3.24x10^{-8}=\frac{x^{2}}{5x10^{-8}-x}$

clearing the <em>x</em>

${x^{2}={1.62x10^{-17}-3.24x10^{-8}x}$

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