14.6 Acid Base Mixing and Titrating

An acid and a base react together and neutralize each other. They always produce:

• CO2 and water

• a salt and water

• CO2 and a salt

• CO2 and O2

• water and O2

What are the two products of HCl and NaOH reacting together?

• H2O

• NaCl

• H3O⁺

• OH^-

• Na₂O

What are the two products of HBr and KOH reacting together?

• H2O

• KBr

• H3O⁺

• OH^-

• K₂O

Calculate the number of moles of H⁺ (which is also H₃O⁺) in beaker 1.

• (0.75)(0.020) = 0.015 mols H⁺

• (0.75)/(0.020) = 37.5 mols H⁺

• (0.020)/(0.75) = 0.0267 mols H⁺

• (0.75)/(20) = 15 mols H⁺

Calculate the number of moles of OH^- in beaker 2.

• (0.85)(0.0195) = 0.0166 mols OH^-

• (0.85)/(0.0195) = 43.6 mols OH^-

• (0.0195)/(0.85) = 0.0229 mols OH^-

• (0.85)/(19.5) = 16.6 mols OH^-

From the previous two questions, you should've calculated 0.0150 mols of H⁺ and 0.0166 mols of OH^-.

How much is left over after they react in a 1:1 mole ratio?

• 0.001575 mols of OH^-

• 0.001575 mols of H⁺

• 0.031575 mols of OH^-

• 0.031575 mols of H⁺

Tags

NGSS.HS-PS1-7

From previous question, you should've calculated 0.001575 mols of OH^- left over. Calculate total volume and find the Molarity of OH-.

Molarity = mols/L

• 0.001575 / 0.0395 = 0.0399 M OH^-

• 0.001575 / 39.5 = 3.99 x 10^-5 M OH^-

• 0.001575 * 0.0395 = 6.22 x 10^-5 M OH^-

• 0.0395 / 0.001575 = 25.1 M OH^-

Using the [OH-] you calculated in the last question, 0.0399 M, calculate the pH of this solution.

• 1.40

• 12.60

• 0.912

• 13.09

When 440 mL of 3.1 M HClO₄ is mixed with 220 mL of 4.1 M LiOH, what is the pH of the resulting solution?

• pH = 0.15

• pH = 0.70

• pH = 0.462

• pH = 0.902

Before a titration experiment is begun, NaOH is filled in the buret until it's a little below the zero. The value is recorded as:

• 1.40

• 2.60

• 1.50

• 2.70

• 1.10