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A 10.00 mL sample of a 1.07 M solution of potassium hydrogen phthalate (KHP, formula mass = 204.22 g/mol) is diluted to 250.0 mL. What is the molarity of the final solution?

Respuesta :

jpelezo1

Answer:

[KHP] = 0.0428M

Explanation:

2 methods to calculate concentration after dilution

1. Use dilution equation

Molarity of concentrate (M₁) x Volume of Concentrate (V₁)

           =    Molarity of dilute (M₂) x Volume of dilute (V₂)

M₁ x V₁ = M₂ x V₂ => M₂ = M₁ x V₁ / V₂ = (1.07M)(10ml)/(250ml) = 0.0428M

2. Concentration Equation

moles KHPh = Molarity (M)  x  Volume (V) = 1.07M x 0.010L =0.0107 moles KHP

Concentration KHP = moles solute / volume of solution in Liters

= 0.0107 moles KHP / 0.25L = 0.0428M

samueladesida43

The molarity of 10.00 mL sample of a 1.07 M solution of potassium hydrogen phthalate diluted to 250.0mL is 0.0428M.

HOW TO CALCULATE MOLARITY:

  • The molarity of a diluted solution can be calculated by using the following formula:

C1V1 = C2V2

Where;

  1. C1 = initial concentration of solution
  2. C2 = final concentration of solution
  3. V1 = initial volume of solution
  4. V2 = final volume of solution

According to this question,

  1. C1 = 1.07M
  2. C2 = ?
  3. V1 = 10.0mL
  4. V2 = 250mL

  • 1.07 × 10 = C2 × 250

  • 10.7 = 250C2

  • C2 = 10.7 ÷ 250

  • C2 = 0.0428M

  • Therefore, the molarity of 10.00 mL sample of a 1.07 M solution of potassium hydrogen phthalate diluted to 250.0mL is 0.0428M.

Learn more about how to calculate molarity of a solution at: https://brainly.com/question/13386686?referrer=searchResults