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3 years ago

The ph of a solution prepared by mixing 45.0 ml of 0.183 m koh and 35.0 ml of 0.145 m hcl is ________.

Chemistry

1 answer:

Naddika [18.5K]3 years ago

4 0

Answer:

12.6.

Explanation:

We should calculate the no. of millimoles of KOH and HCl:

no. of millimoles of KOH = (MV)KOH = (0.183 M)(45.0 mL) = 8.235 mmol.

no. of millimoles of HCl = (MV)HCl = (0.145 M)(35.0 mL) = 5.075 mmol.

It is clear that the no. of millimoles of KOH is higher than that of HCl:

So,

[OH⁻] = [(no. of millimoles of KOH) - (no. of millimoles of HCl)] / (V total) = (8.235 mmol - 5.075 mmol) / (80.0 mL) = 0.395 M.

∵ pOH = -log[OH⁻]

∴ pOH = -log(0.395 M) = 1.4.

∵ pH + pOH = 14.

∴ pH = 14 - pOH = 14 - 1.4 = 12.6.

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Likurg_2 [28]

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The chemical reaction has been defined as the interaction of the reactant molecules for the formation of the product. The changes have been taken place in the reactivity series and under specific conditions.

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The displacement reaction has been taken place based on the reactivity series. The more reactive element has been able to displace the less reactive element in the compound and form a new compound.

The following reactions have been analyzed as:

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In the reaction, Al has been replaced by Fe. The Fe is more reactive than Al. thus this reaction will occur.

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3 years ago

Temperature is an example of a categorical variable a quantitative variable either a quantitative or categorical variable neithe

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Answer: Temperature is an example of a quantitative variable

Explanation:

A quantitative variable is defined as :

A variable that can assume a numerical value .
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Temperature comes under interval scale , because interval scale has no zero point.

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3 years ago

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We'll begin by calculating the number of mole of in 0.16 g of Ca(OH)₂. This can be obtained as follow:

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Mole = mass / molar mass

Mole of Ca(OH)₂ = 0.16 / 74

Next, we shall determine the molarity of the stock solution of Ca(OH)₂.

Mole of Ca(OH)₂ = 0.00216 mole

Volume = 100 mL = 100 / 1000 = 0.1 L

<h3>Molarity of Ca(OH)₂ =? </h3>

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Next, we shall determine the molarity of the diluted solution. This can be obtained as follow:

Volume of stock solution (V₁) = 100 mL

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0.0216 × 100 = M₂ × 250

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M₂ = 2.16 / 250

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