1. It requires 25.05 mL of NaOH solution of unknown concentration to titrate 25.

ID: 830332 • Letter: 1

Question

1. It requires 25.05 mL of NaOH solution of unknown concentration to titrate 25.00 mL of 0.1000 M H2SO4 solution. The chemical equation that summarizes the reactio is H2SO4 + 2NaOH --> 2H2O + Na2SO4. Calculate the concentration of the NaOH solution.

2. Suppose we add 30.0 mL of .100 M NaOH to 50.0 mL of 0.100 M HCl. Calculate the concentration of the remaining acid that was not neutralized. what is the pH of the solution?

3. Naphthalene normally freezes at 80.2 degrees C and has a Kf value of 6.9 C/m. A solution containing 1.19 g of sulfer dissolved in 10.20 g of naphthalene freezes at 77.1 degrees C. Calculate the molality of the solution and the molar mass of the solute, sulfer.

Explanation / Answer

1)25.05*C=25*0.2

C(NaOH)=0.197M

2. Suppose we add 30.0 mL of .100 M NaOH to 50.0 mL of 0.100 M HCl. Calculate the concentration of the remaining acid that was not neutralized. what is the pH of the solution?

2)moles of acid=0.05L*0.1moles/L=0.005moles

moles of base=0.003moles

moles of acid remainng=0.005-0.003=0.002moles

Molarity of acid=0.002moles/0.08L=0.025M

pH=-log[H+]=-log(0.025)=1.6

c)Molality=moles of solute/kg of solvent=1.19gsulfer/0.0102kg naphthalene

=(1.19g/32g/mole)/0.0102kg naphtha=0.0372moles of sulfer/0.0102Kg naphtha

=3.65molal

(Note: molar mass of solute sulfer is 32g/mole)

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1. It requires 25.05 mL of NaOH solution of unknown concentration to titrate 25.

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