1. What is the concentration (in M) of an aqueous solution of sulfuric acid prep

Question

1. What is the concentration (in M) of an aqueous solution of sulfuric acid prepared by transferring 25.0 mL of 6.00 M H2So4(aq) to a 250 mL-volume volumetric flask that is subsequently filled to its 250 mL-mark with distilled water? 2. What volume of a saturated solution of 8.43 M KI(aq) at 20 C is needed to form 10.0 L of a 1.00 M solution? What volume of pure water is needed as diluent? 3. Identify the type of electrolyte (strong, weak, or non- formed when the following compounds dissolve in pure water. a) Ethylamine (CH3CH2NH2, an organic base) b) Calcium fluoride c) Argon d) oxygen e sodium hydroxide Hexanoic acid 4. Which one of the following solutions is the best conductor of electricity? A. 1 M NaCl B. 1 M NH C. 1 M CH30H D. 1 M CH3COOH E. They all conduct electricity equally well

Explanation / Answer

Volume of H2SO4 intially V1 = 25 mL = 0.025 L

Molarity of  H2SO4 intially M1 = 6 M (or mol/L)

No. of moles of H2SO4 = V1* M1 = 0.025 L * 6 mol/L = 0.15 moles of H2SO4

same no. of moles of H2SO4 will be present after adding Distilled water to make it to 250 mL = 0.25 L

so Molarity = No. of moles / volume in L = 0.15 moles / 0.25 L = 0.6 mol/L or 0.6 M Answer

Given we need 10 L of 1 M of KCl

so no of moles need to be present = 10 L * 1 mol/L = 10 moles

we have solution of 8.34 M(or mol/L)

so volume of KCl of orginal solution required = No. of moles /Molarity of orginal solution = 10 mol / 8.34 mol/L = 1.12 L

so we require 1.12 L of KCl answer

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