7.0 mL of 3.0 M NaOH are diluted wit the resulting solution h water to a volume

Question

7.0 mL of 3.0 M NaOH are diluted wit the resulting solution h water to a volume of 400 mL Determine the molarity of a. How many moles of NaOH there are in 7.0 mL of 3.0 M NaOH? Hint: Use Eq. 1 and make sure the volume is in liters. _moles moles of NaOH is not changed on dilution. The molarity after dilution b. The total number of can therefore be found by Eq. 1, using the final volume of the solution. Calculate that molarity. In an acid-base titration, 25.62 mL of an NaOH solution are needed to neutralize 26.23 mL of a 0.1036 M HCI solution. Use these steps to find the molarity of the NaOH. 2. a. First note the value of M in the HCI solution. b. Find MoH- in the NaOH solution. (Use Eq. 3.) LM c. Obtain MNaOH from MoH-

Explanation / Answer

1. NaOH dilution

a. moles NaOH in 7.0 ml (0.007 L) = 3.0 m x 0.007 L = 0.021 moles

b. molarity of NaOH after dilution (0.4 L) = 0.021 moles/0.4 L = 0.0525 M

2. neutralization of NaOH with HCl

a. moles HCl used = 0.1036 M x 26.23 ml = 2.72 mmol

b. moles NaOH present = 2.72 mmol

c. molarity of NaOH solution = 2.72 mmol/25.62 ml = 0.1062 M

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