Question


What is the pH of a 8.6 x 10-8 M solution of HCl(aq) at 25 °C? Report your answer to the hundredths place. pH =
Assuming complete dissociation, what is the pH of a 3.98 mg/L Ba(OH), solution? pH = X10
Assuming equal concentrations, arrange these solutions by pH. Highest pH Lowest pH Answer Bank HCIO, (aq) Cabr,(aq) NaCN(aq)
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Answer #1

1)

HCl is strong acid , so completely dissociates.

Concentration of HCl = Concentration of H3O+

[H3O+] = 8.6 ×10-8M

pH = -log[H3O+]

pH = -log( 8.6×10-8)

pH = 7.07

2)

Mole = mass/molar mass

moles of Ba(OH)2 = 0.00398g/171.35g/mol = 2.323×10-5mol

moles of OH- = 2 × 2.323×10-5mol = 4.646 ×10-5mol

molarity of OH- = 4.646×10-5mol/L

pOH = -log[OH-]

pOH = - log( 4.646×10-5mol/L)

pOH = 4.33

pH = 14 - pOH

pH = 14 - 4.33

pH = 9.67

3)

Highest pH

RbOH(aq)

NaCN(aq)

CaBr2(aq)

CH3NH3Br(aq)

HClO4(aq)

Lowest pH

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