Question

**Part A:**

0.65 g of hydrogen chloride (HCl) is dissolved in water to make 8.0 L of solution. What is the pH of the resulting hydrochloric acid solution?

**Part B:**

0.20 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 3.0 L of solution. What is the pH of this solution?

Answer #1

**Part A :**

*Given data,*

*Mass of HCl = 0.65 g*

*Volume = 8.0 L*

*Molar mass of HCl = 36.5 g per mol*

*Moles of HCl = mass / Molar mass*

*= 0.65 g / 36.5 g per mol*

**Moles of HCl = 0.0178 mol**

*Molarity = moles / volume in liter*

*= 0.0178 / 8.0 L*

*= 0.00222 M*

*Now calculate the pH,*

*pH = - log [H ^{+}]*

*= - log [0.00222]*

*= - ( -2.65 )*

**pH = 2.65**

**PartB:**

*Given data, mass = 0.20 g*

*molar mass of NaOH = 40 g/mole*

*Moles of NaOH = mass / molar mass of NaOH*

*= 0.20 / 40*

*= 0.005 mol*

*[OH ^{-}] = [NaOH] = moles of NaOH / volume*

*= 0.005 / 3*

*= 0.00166 M*

*p ^{OH} = -log[OH^{-}]*

*= -log[0.00166]*

*= 2.77*

*p ^{H} = 14 - p^{OH}*

*= 14 - 2.77*

**p ^{H} = 11.23**

Part A
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Part B
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Express the pH numerically to two decimal places.
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0.25 g of hydrogen chloride (HCl) is dissolved in water to make
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Part B
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Express the pH numerically to two decimal places
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