Concentration Units and Conversion Factors
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Questions and Answers

What is the mass of NaCl required to prepare 250 mL of a 0.92% (w/v) NaCl solution?

  • 2.3 g (correct)
  • 1.5 g
  • 4.6 g
  • 3.5 g

    • What is the concentration of a solution in parts per million if 0.0054 g of MgCl2 is dissolved in 2000 g of solvent?

  • 5.4 ppm
  • 2.7 ppm (correct)
  • 2.7 ppm (correct)
  • 10.8 ppm

    • What is the molarity of a solution made from 20.0 g of NaOH in 250 mL of solution?

  • 0.75 M
  • 0.50 M (correct)
  • 0.25 M
  • 1.00 M

    • What is the weight/volume percent concentration of a solution that contains 2.3 g of NaCl in 250 mL of solution?

    <p>0.92%</p> Signup and view all the answers

    What is the unit of concentration that represents the number of moles of solute per liter of solution?

    <p>Molarity</p> Signup and view all the answers

    What is the concentration of a solution that contains 0.92 g of NaCl in 100 mL of solution?

    <p>0.92% (w/v)</p> Signup and view all the answers

    What is the equivalent weight of CaBr2?

    <p>99.945 g/mol</p> Signup and view all the answers

    How is the concentration of a solution often expressed when it contains a very small concentration of solute?

    <p>Parts per Million</p> Signup and view all the answers

    What is the normality of a 0.4 g/100 mL solution of CaBr2?

    <p>0.02 N</p> Signup and view all the answers

    What is the weight/volume percent concentration of a solution that contains 20 g of solute in 100 mL of solution?

    <p>20% (w/v)</p> Signup and view all the answers

    What is the purpose of a conversion factor in solution chemistry calculations?

    <p>To cancel units</p> Signup and view all the answers

    How many milliequivalents of Ca2+ are present in 0.4 g of CaBr2?

    <p>4 mEq</p> Signup and view all the answers

    What is the volume/volume percent concentration of a solution that contains 30 mL of solute in 100 mL of solution?

    <p>30% (v/v)</p> Signup and view all the answers

    How many grams of NaCl are contained in 500 mL of a 0.92% (w/v) NaCl solution?

    <p>9.2 g</p> Signup and view all the answers

    What is the concentration of a solution that contains 25 g of solute in 200 mL of solution?

    <p>12.5% (w/v)</p> Signup and view all the answers

    How many milliequivalents of Ca2+ are present in 0.2 g of CaBr2?

    <p>2 mEq</p> Signup and view all the answers

    What is the amount of each ion in 1 mole of solution that relates to its charge?

    <p>Equivalent</p> Signup and view all the answers

    How many equivalents are present in 0.5 mol of PO43-?

    <p>1 Eq</p> Signup and view all the answers

    What is the concentration unit used to express the amount of ions in body fluids?

    <p>Milliequivalents per liter</p> Signup and view all the answers

    How many milliequivalents are there in 1 equivalent?

    <p>1000 mEq</p> Signup and view all the answers

    What is the number of positive ions always equal to in a neutral solution?

    <p>Number of negative ions</p> Signup and view all the answers

    How many moles of magnesium ion are in 0.4 L of blood with a magnesium level of 16.0 mEq/L?

    <p>0.016 mol</p> Signup and view all the answers

    What is the amount of calcium ion in 0.4 g of CaBr2?

    <p>0.4/2 mEq</p> Signup and view all the answers

    What is the type of electrolyte that ionizes completely in solution?

    <p>Strong electrolyte</p> Signup and view all the answers

    Study Notes

    Concentration Units

    • A 0.92% (w/v) NaCl solution is equivalent to 0.92 g NaCl per 100 mL of solution.
    • To find the mass of NaCl in 250 mL of solution, use the conversion factor: 0.92 g NaCl / 100 mL solution.

    Parts Per Million (ppm)

    • ppm = (mass of solute (g) x 10^6) / mass of solution (g)
    • ppm = (volume of solute (mL) x 10^6) / volume of solution (mL)
    • Example: 0.0054 g of MgCl2 in 2000 g of solvent.

    Molarity (M)

    • Molarity is the number of moles of solute per liter of solution.
    • M = moles of solute (mol) / liter of solution (L)
    • Example: 20.0 g of NaOH in 250 mL of solution.

    Weight/Volume Percent Concentration (w/v)%

    • w/v% = (mass of solute (g) / volume of solution (mL)) x 100%
    • Example: 5 g of acetic acid in 100 mL of solution is 5% w/v.

    Volume/Volume Percent Concentration (v/v)%

    • v/v% = (volume of solute (mL) / volume of solution (mL)) x 100%
    • Example: 70 mL of 2-propanol in 100 mL of solution is 70% v/v.

    Electrolytes

    • Strong electrolytes: ionize completely in solution (e.g., NaCl → Na+ + Cl-)
    • Weak electrolytes: ionize partially in solution (e.g., CH3COOH → H+ + CH3COO-)

    Equivalents (Eq)

    • Equivalent (Eq) is a unit used to express the amount of each ion in solution.
    • Amount of ion in solution is determined by equivalent (Eq), which relates to its charge.

    Milliequivalents (mEq)

    • 1 Eq = 1000 mEq
    • Concentration of ions in the body is determined by mEq/L.

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    Description

    Solve a problem involving concentration units and conversion factors, given a 0.92% NaCl solution and 250 mL volume. Apply conversion factors to find the desired quantity of NaCl.

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