1. What is the molarity of a copper(II) dihydroxide [Cu(OH)2] solution if 25.25 mL of the solution is titrated to the equivalence point with 36.18 mL of 0.549 M prussic acid [H(CN)]?

2. What volume of a 0.138 M dihydroxyl base solution is needed to neutralize 28.47 mL of 0.745 M triprotic acid?

3. How many mL of 2.57 M Pb(OH)2 are necessary to neutralize 15.6 mL of each of the following acids?
A. 1. 39 M H(MnO4)

B. 2.37 M H2(C2O4)

C. 0. 739 M H3(PO4)

4. What is the molarity of a Li(OH) solution if 45. 30 mL is required to neutralize 27. 90 mL of a 1.52 M solution of H(NO3) ?

5. Calculate the volume in mL of a 0. 680 M solution of H(ClO3) that is necessary to neutralize 32. 58 mL of a 0.1254 M solution of K(OH).

6. In a titration involving Mg(OH)2, it took 51.78 mL of Mg(OH)2 to neutralize 27.34 mL of 0.478 M H2(CrO4). What is the molarity of the Mg(OH)2?

7. In a titration of HCl with Na(OH), what volume of a 8.5 M solution of Na(OH) would it take to neutralize 17.20 mL of 12.0 M HCl?

8. It requires 56.74 mL of Ti(OH)2 solution to neutralize 49.87 mL of 0. 8121 M H2(SO3). What is the concentration of the potassium hydroxide solution?

Is there a balanced eq. with this ??

0.0243L NaOH

To solve these problems, you will need to use the concept of titration. In titration, a solution of known concentration, called the titrant, is added to a solution of unknown concentration until the reaction between the two solutions is complete. From this information, you can determine the concentration of the unknown solution.

Here's a step-by-step breakdown on how to solve these titration problems:

1. Determine the balanced chemical equation for the reaction of interest. For example, in problem 1, the reaction between copper(II) dihydroxide [Cu(OH)2] and prussic acid [H(CN)] can be represented as:
Cu(OH)2 + 2 H(CN) → Cu(CN)2 + 2 H2O

2. Use stoichiometry to determine the mole ratio between the reactants in the balanced equation. In this example, 1 mol of Cu(OH)2 reacts with 2 mol of H(CN).

3. Determine the number of moles of the known solution (titrant) using the given concentration and volume. Use the formula: moles = concentration (in M) x volume (in L). For example, in problem 1, the number of moles of H(CN) is calculated as:
moles H(CN) = 0.549 M x 0.03618 L

4. Use the mole ratio from step 2 to determine the number of moles of the unknown solution (analyte). In this example, the number of moles of Cu(OH)2 is twice the number of moles of H(CN).

5. Determine the volume of the unknown solution using the number of moles and the molarity. Use the formula: volume (in L) = moles / concentration (in M). For example, in problem 1, the volume of Cu(OH)2 solution can be calculated as:
volume Cu(OH)2 = (2 moles H(CN) / 2) / molarity Cu(OH)2

6. Finally, convert the volume to mL if necessary by multiplying by 1000. For example, the volume in mL for problem 1 would be 25.25 mL.

Repeat these steps for each of the given problems, adjusting the specific balanced equation and molar ratios accordingly.