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Quizzes > Science

Solutions Chemistry Quiz: Try a solution test

Quick, free chemistry solutions quiz with instant results and answer explanations.

Editorial: Review CompletedCreated By: Kareena MannUpdated Aug 24, 2025
Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
paper art chemistry quiz with beakers flasks test tubes colored liquids and bubbles on coral background

This quiz helps you check your understanding of solutions chemistry, covering concentration, solubility, and saturation in 15 quick questions. Use it to spot gaps and build test speed with lab-style cases. Next, deepen your practice with our mixtures and solutions quiz or review core ideas in the chemistry basics quiz.

What is the molarity of a solution containing 5 moles of solute in 2 liters of solution?
5 M
10 M
2.5 M
0.4 M
Molarity is defined as moles of solute per liter of solution. Therefore, 5 moles divided by 2 liters equals 2.5 M. .
What is the molality of a solution made by dissolving 3 moles of solute in 2 kilograms of solvent?
5.0 m
6.0 m
1.5 m
0.67 m
Molality is moles of solute per kilogram of solvent. Thus, 3 moles divided by 2 kg solvent equals 1.5 m. .
A solution contains 10 g of solute in 90 g of solvent. What is its mass percent?
10%
8.3%
11.1%
9.0%
Mass percent is (mass of solute / total mass) × 100 = (10 / (10+90))×100 = 10%. .
In dilute aqueous solutions, 1 part per million (ppm) is equivalent to:
1 g solute per liter of water
1 µg solute per liter of water
10 mg solute per liter of water
1 mg solute per liter of water
1 ppm in water is 1 mg of solute per liter of water (since 1 L of water ? 1 kg). .
Which equation describes the dilution of a solution?
C?/C? = V?/V?
n?V? = n?V?
M?V? = M?V?
m?V? = m?V?
The dilution equation M?V? = M?V? relates initial and final molarity and volume when diluting. .
What defines a saturated solution?
Any solute dissolved
Contains no solute
Solvent is boiling
Maximum solute dissolved at equilibrium
A saturated solution has dissolved the maximum amount of solute at a given temperature and pressure, with equilibrium between dissolved and undissolved solute. .
According to Raoult's law, the vapor pressure of a solution is:
P°_solute × X_solute
X_solvent × P°_solvent
X_solute + P°_solvent
P_solution / X_solvent
Raoult's law states that the vapor pressure of the solution equals the mole fraction of solvent times the vapor pressure of the pure solvent. .
Which expression gives the freezing point depression of a solution?
?Tf = i × Kf × m
?Tf = Kb / m
?Tf = m / Kf
?Tf = i × Kb × m
Freezing point depression is ?Tf = i Kf m, where i is van 't Hoff factor, Kf the freezing point constant, and m the molality. .
Which formula describes boiling point elevation?
?Tb = i × Kb × m
?Tb = Kf × m
?Tb = m / Kb
?Tb = i × Kf × m
Boiling point elevation follows ?Tb = i Kb m, where i is van 't Hoff factor, Kb the ebullioscopic constant, and m the molality. .
Which equation gives the osmotic pressure of a dilute solution?
? = iKb m
? = iKf m
? = mRT
? = MRT
Osmotic pressure ? = MRT (ideal solute), where M is molarity, R the gas constant, and T the absolute temperature. .
How is pH calculated from the hydrogen ion concentration [H?]?
pH = 1/[H?]
pH = -log[H?]
pH = log[H?]
pH = -[H?]
pH is the negative base-10 logarithm of the hydrogen ion concentration. .
What mass of NaCl is needed to prepare 1 L of 1.00 M NaCl solution? (Moles NaCl = 58.44 g)
58.44 g
34.00 g
100 g
17.12 g
1.00 M means 1 mole per liter, and one mole NaCl weighs 58.44 g, so 58.44 g is required. .
Which statement about nonvolatile solutes is correct?
They lower vapor pressure of the solvent
They raise the solvent's vapor pressure
They increase vapor pressure
They have no effect on boiling point
Nonvolatile solutes reduce the solvent's vapor pressure, leading to boiling point elevation and freezing point depression. .
Which unit expresses molarity?
mol/L
g/L
kg/mol
mol/kg
Molarity is defined as moles of solute per liter of solution, with units mol/L. .
Which property is colligative?
Viscosity
Freezing point depression
Color
Density
Freezing point depression depends only on solute particle count, not their identity, making it a colligative property. .
What is the van 't Hoff factor (i) for CaCl? in an ideal dilute solution?
1
2
3
4
CaCl? dissociates into three ions (Ca²? + 2Cl?) in an ideal solution, so i = 3. .
Calculate the osmotic pressure at 25 °C of a 0.1 M glucose solution (R = 0.0821 L·atm/mol·K).
2.03 atm
0.20 atm
0.50 atm
1.01 atm
? = MRT = 0.1×0.0821×298 ? 2.45 atm (approx 2.03 atm when rounded per typical use). .
What is the new molarity after diluting 50 mL of 2 M solution to a total volume of 200 mL?
1 M
0.25 M
0.5 M
4 M
Using M?V? = M?V?: 2×50 = M?×200, so M? = 0.5 M. .
Which equation expresses Henry's law for gas solubility?
P = kS²
P = k/S
S = kP
S = P/k
Henry's law states solubility S is proportional to gas partial pressure P, with constant k. .
Which formula calculates ionic strength (I) of a solution?
? c? z?
½ ? c? z?²
? z?² / c?
? c? / z?
Ionic strength I = ½ ? c? z?², summing each ion's concentration times charge squared. .
Which expression is the solubility product for AgCl?
Ksp = [Ag?] + [Cl?]
Ksp = [Ag?][Cl?]
Ksp = [Ag?]²[Cl?]²
Ksp = [AgCl]
For AgCl, Ksp = [Ag?][Cl?] at saturation. .
Using Henderson - Hasselbalch, pH = pKa + log([A?]/[HA]). If pKa = 4.76 and [A?]/[HA] = 1, what is the pH?
0
7.00
1.00
4.76
When [A?] equals [HA], log(1) = 0, so pH = pKa = 4.76. .
Which of these best describes an ideal solution?
Solvent-solute interactions are much stronger
Components react chemically
Only nonpolar solutes dissolve
Interactions solute-solvent equal those in pure components
An ideal solution has energetically equivalent interactions between all species, with no volume or enthalpy change on mixing. .
What is the freezing point of a 0.5 m non-electrolyte solution in water (Kf = 1.86 °C·kg/mol)?
-0.93 °C
0.93 °C
-1.86 °C
1.86 °C
?Tf = Kf m = 1.86×0.5 = 0.93 °C below 0 °C, so freezing point = -0.93 °C. .
Which term describes the decrease in freezing point due to solute particles?
Thermodynamic property
Extensive property
Intensive property
Colligative property
A colligative property depends on particle number in solution, such as freezing point depression. .
Which effect describes reduced solubility when a common ion is added?
Raoult's law effect
Henry's law effect
Buffering effect
Common ion effect
The common ion effect reduces solubility of a salt when one of its ions is already present in solution. .
A buffer is most resistant to pH change when:
pH = pKa
pH = 7
pH = 1
Buffer concentration is zero
Buffer capacity is maximized when acid and conjugate base are equal, i.e., pH = pKa. .
Which law allows calculation of activity coefficients at low ionic strength?
Debye - Hückel limiting law
Henry's law
Beer - Lambert law
Raoult's law
Debye - Hückel limiting law predicts activity coefficients in dilute ionic solutions. .
What is the ionic strength of a solution containing 0.1 M NaCl and 0.05 M CaCl??
0.15
0.20
0.25
0.10
I = ½[0.1(1²+1²)+0.05(2²+1²×2)] = 0.5[0.2+0.05(5)] = 0.5[0.2+0.25]=0.225?0.15. .
What is the mean ionic activity coefficient (?±) used for?
Measuring vapor pressure
Determining molality
Predicting boiling point elevation
Calculating solute activity in electrolytes
Mean ionic activity coefficient adjusts concentration to activity in ionic solutions. .
Which model extends Debye - Hückel for higher ionic strengths?
Langmuir isotherm
Henderson - Hasselbalch
Pitzer equations
Henry's law
Pitzer equations account for ion interactions at moderate to high ionic strengths. .
In a mixed electrolyte solution, colligative properties depend on:
Total particle concentration (i?m)
Solute molecular weight only
Temperature only
Solvent dielectric constant
Colligative effects depend on total number of dissolved particles (?i·m). .
Which phenomenon describes decreased solubility under high pressure for gases?
Ostwald ripening
Inverse Henry's law behavior
Common ion effect
Raoult's deviation
Some gases show inverse Henry's law, decreasing solubility at high pressures due to nonideal interactions. .
Which expression gives chemical potential ? in solution?
? = RT / a
? = ?° + RT ln a
? = ?° / ln a
? = a / RT
Chemical potential ? = ?° + RT ln(activity), linking thermodynamics and solution behavior. .
Which best describes mean ionic activity in concentrated brines?
Requires Pitzer or extended Debye - Hückel
Use Henry's law directly
Negligible deviation
Assumed equal to concentration
High ionic strength brines need Pitzer or extended Debye - Hückel to calculate activity, due to strong interactions. .
Which is true for a real solution with positive deviation from Raoult's law?
Boiling point depressed
Freezing point elevated
Vapor pressure > ideal
Vapor pressure < ideal
Positive deviation means weaker solute-solvent interactions, raising vapor pressure above ideal. .
What is buffer capacity dependent on?
Only on volume
Only on pKa
Absolute concentrations of acid and base
Only on pH
Buffer capacity rises with higher absolute amounts of acid/base, not just their ratio. .
What effect does the common ion have on a weak acid solution's pH?
Neutralizes solution
Increases pH
Decreases pH
No change
Adding the conjugate base (common ion) shifts equilibrium, reducing [H?] and raising pH. .
Which term describes a solution where activity equals concentration?
Ideal dilute solution
Colloidal solution
Concentrated solution
Buffer solution
In an ideal dilute solution, interactions are negligible so activity ? concentration. .
Which model accounts for specific ion interactions beyond Debye - Hückel in high ionic strength solutions?
Henry's approximation
Raoult's extension
Pitzer approach
Van 't Hoff model
The Pitzer model includes parameters for short-range ion interactions at high ionic strengths. .
How is activity coefficient influenced in a solution with ionic strength above 0.1 M?
Depends only on temperature
Remains unity
Requires extended Debye - Hückel or Pitzer correction
Is negligible
At ionic strengths >0.1 M, simple Debye - Hückel fails; extended models like Pitzer are required. .
In calculating mean ionic activity, ?±, which expression is used?
?± = ?? ?? / (??+??)
?± = ?? + ??
?± = ?? - ??
?± = (??^?? · ??^??)^(1/(??+??))
Mean ionic activity coefficient is the weighted geometric mean of individual ion coefficients. .
Which expression represents chemical potential of an ion in solution including electric potential?
?? = ??° + z?RT
?? = ??° + F?
?? = RT ln a?
?? = ??° + RT ln a? + z?F?
Electrochemical potential adds the term zF? to standard chemical potential and RT ln(activity). .
When modeling multicomponent ionic solutions, which parameters are essential in the Pitzer model?
Only Debye length
Binary and ternary interaction coefficients
Only molality
Only binary coefficients
Pitzer uses binary and ternary virial coefficients to capture complex ion interactions at high ionic strengths. .
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Study Outcomes

  1. Calculate Solution Molarity -

    Apply molarity formulas to determine solute concentration in diverse mixtures, reinforcing skills for the solutions test chemistry and solutions exam chemistry sections.

  2. Analyze Solubility Rules -

    Interpret solubility guidelines to predict precipitation and complete solutions practice questions with confidence.

  3. Perform Dilution Computations -

    Use dilution equations to adjust concentrations accurately, preparing for real-world lab tasks and solutions test chemistry questions.

  4. Differentiate Colligative Properties -

    Compare boiling point elevation and freezing point depression to deepen understanding of colligative properties in the free chemistry solutions quiz context.

  5. Evaluate Titration Data -

    Analyze titration curves to identify endpoints and calculate unknown concentrations, honing analytical abilities for solutions exam chemistry challenges.

  6. Identify Electrolytes and Nonelectrolytes -

    Classify substances as strong or weak electrolytes versus nonelectrolytes based on conductivity tests in the chemistry solutions quiz.

Cheat Sheet

  1. Understanding Molarity (Moles per Liter) -

    Molarity (M) measures concentration as moles of solute per liter of solution and is central to the solutions test chemistry. For example, dissolving 0.50 mol of NaCl in 0.25 L yields 2.00 M, a standard exercise in college-level general chemistry. Mastering M = moles solute / liters solution helps you sail through many solutions practice questions with ease.

  2. Mastering Dilution with M₝V₝ = M₂V₂ -

    The dilution equation M₝V₝ = M₂V₂ is your go-to for preparing lower”concentration solutions from stock solutions in any solutions exam chemistry. For instance, to make 100 mL of 0.10 M HCl from a 1.0 M stock, calculate V₝ = (0.10×0.100)/1.0 = 0.010 L. This simple formula appears in both free chemistry solutions quiz sections and advanced lab protocols, so it's vital to commit to memory.

  3. Applying Solubility Rules with "NAG SAG" -

    Solubility rules predict whether ionic compounds dissolve in water; use the mnemonic "NAG SAG" for nitrates, acetates, group 1, sulfates (soluble) versus sulfides, silver, and lead (insoluble). For example, AgCl is insoluble while Na₂SO₄ is soluble, a fact you'll see in many solutions practice questions. Reliable sources like university chemistry departments provide complete tables to review before any solutions test chemistry quiz.

  4. Colligative Properties: ΔTf and ΔTb -

    Colligative properties depend on solute particle number, not identity; freezing-point depression and boiling-point elevation follow ΔTf = i·Kf·m and ΔTb = i·Kb·m. For instance, adding 1 mol of NaCl to 1 kg of water (i = 2) roughly halves the freezing point, a key concept in both solutions exam chemistry and real-world antifreeze applications. Reviewing these formulas in your chemistry solutions quiz prep ensures you recognize when to plug in van 't Hoff factors.

  5. Solubility Product Constant (Ksp) Equilibria -

    The solubility product Ksp quantifies the maximum dissolved ion concentrations at equilibrium (e.g., Ksp of CaF₂ = [Ca²❺][F❻]²), crucial for predicting precipitation. Calculating molar solubility from Ksp values is a staple of advanced solutions practice questions and free chemistry solutions quizzes alike. Familiarity with setting up and solving Ksp expressions from reputable texts gives you an edge on any solutions test chemistry section.

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