Unlock hundreds more features
Save your Quiz to the Dashboard
View and Export Results
Use AI to Create Quizzes and Analyse Results

OR
Sign inSign in with Facebook
Sign inSign in with Google
Quizzes > Science > Chemistry

KCl Solubility at 50°C Quiz: Can You Master Saturation?

Think you know about a supersaturated solutionn for nano3 at the temprature for 50c? Take the test now!

Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
Paper art design shows KCl solubility quiz at 50 C with supersaturated NaNO3 and solubility graphs on dark blue background

Calling all budding chemists and curious minds! Dive into our free solubility quiz designed to help you master the concept that a solution of kcl is saturated at 50 c and challenge your expectations on a supersaturated solutionn for nano3 at the temprature for 50c. Compare behavior of a supersaturated solution for nano3 at a tempature of 5c while applying table G solubility levels in solutions. Armed with clear insights on saturation in chemistry from our guide , you'll test solubility knowledge, reinforce solubility rules trivia and sharpen your lab-ready skills. Ready to push the limits of your chemistry prowess? Click to start now.

What is the approximate solubility of KCl in 100 g of water at 50 °C?
45.8 g
32.0 g
60.2 g
25.4 g
At 50 °C, KCl dissolves to about 45.8 g per 100 g water, as shown in standard solubility tables. This value is widely referenced in chemical handbooks. Temperature strongly influences this value, with lower temperatures giving lower solubility. Chemguide: Solubility
How does the solubility of KCl change as temperature increases from 20 °C to 50 °C?
It increases
It decreases
It remains constant
It first decreases then increases
For most salts like KCl, solubility increases with temperature due to endothermic dissolution. The solubility curve for KCl slopes upward. Higher thermal energy overcomes lattice energy enabling more solute dissolution. Wikipedia: Solubility
What term describes a solution that contains more dissolved KCl than the saturation point at 50 °C?
Supersaturated
Unsaturated
Saturated
Colloidal
A supersaturated solution holds more solute than its equilibrium solubility at a given temperature. It is a metastable state that can precipitate rapidly if disturbed. Supersaturation is key in crystal growth studies. Wikipedia: Supersaturation
Which salt's solubility is the primary focus of this quiz at 50 °C?
Potassium chloride (KCl)
Sodium chloride (NaCl)
Calcium chloride (CaCl2)
Magnesium sulfate (MgSO4)
The quiz title and content center on KCl solubility at 50 °C. While other salts have their own solubility behaviors, KCl's curve is specifically addressed here. Understanding KCl helps generalize concepts of solubility. PubChem: KCl
What happens when a seed crystal is added to a supersaturated KCl solution at 50 °C?
Rapid crystallization occurs
Solution becomes unsaturated
Temperature drops sharply
Solution turns cloudy due to colloids
Introducing a seed crystal provides a nucleation site, triggering rapid crystallization and precipitation from a supersaturated solution. The excess solute deposits onto the seed until equilibrium is restored. Wikipedia: Nucleation
Which unit is commonly used to express the solubility of KCl in water?
g of solute per 100 g of water
mL of solute per liter of solution
mol of solute per mol of solvent
kg of solution per liter
Solubility tables often use grams of solute per 100 g of solvent to allow easy interpolation. This unit clearly shows how much solute dissolves in a fixed mass of water at a given temperature. LibreTexts: Solubility Units
Compared to its solubility at 20 °C, at 50 °C KCl is:
More soluble
Less soluble
Equally soluble
Undissolvable
Solubility of KCl rises from about 34 g/100 g water at 20 °C to 45.8 g/100 g at 50 °C. Thus, higher temperature dissolves more salt. This trend is typical for endothermic dissolutions. Engineering Toolbox
True or False: Solubility of most ionic salts increases with temperature.
True
False
Most ionic solids have endothermic dissolution, so higher temperatures increase solubility by favoring the dissolution reaction. Some salts are exceptions, but KCl follows the general trend. LibreTexts: Endothermic Reactions
What is the primary factor determining KCl solubility at 50 °C?
Temperature of the solvent
Atmospheric pressure
Color of the container
Agitation speed
Temperature directly affects solubility of solids in liquids by altering kinetic energy and equilibrium. Pressure effects are negligible for solids in water. Container color and stirring only affect dissolution rate, not equilibrium solubility. Wikipedia: Solubility
If a solution contains 30 g of KCl in 100 g water at 50 °C, its saturation status is:
Unsaturated
Saturated
Supersaturated
Precipitated
Since the saturation point at 50 °C is 45.8 g/100 g water, dissolving only 30 g leaves room for more solute, making the solution unsaturated. A saturated solution would contain exactly 45.8 g. Essential Chemical Industry
Compared to KCl, the solubility curve of NaNO3 vs. temperature is:
Steeper slope
More horizontal
Identical
Decreasing with temperature
NaNO3 solubility increases more sharply with temperature than KCl, indicating a steeper solubility curve. This makes NaNO3 easier to supersaturate over a range. Wikipedia: Sodium Nitrate
What is the approximate solubility of NaNO3 at 50 °C?
85 g per 100 g water
45 g per 100 g water
60 g per 100 g water
30 g per 100 g water
At 50 °C, NaNO3 dissolves to about 85 g per 100 g water, much higher than KCl's 45.8 g. This difference underlies its common use in thermal energy storage. Engineering Toolbox
Which principle explains why adding a common ion decreases the solubility of KCl?
Common ion effect
Le Chatelier's principle only
Henry's law
Raoult's law
The common ion effect states that solubility of a salt decreases when a common ion is added, shifting the dissolution equilibrium toward the solid. Le Chatelier's principle also underlies this behavior, but the effect is specifically termed the common ion effect. Wikipedia: Common Ion Effect
When a saturated KCl solution at 50 °C cools to 25 °C, approximately how many grams of KCl precipitate from 100 g water?
20 g
10 g
30 g
45 g
Solubility at 50 °C is ~45.8 g/100 g water, and at 25 °C about 25.5 g/100 g. The difference (~20.3 g) precipitates upon cooling. This principle is used in recrystallization. Chemguide
What effect does pressure have on the solubility of solid KCl in water at 50 °C?
Negligible effect
Doubles solubility
Halves solubility
Reverses solubility curve
Pressure has minimal influence on solubility of solids in liquids because solids and liquids are nearly incompressible. Gas solubility is more pressure-dependent. Wikipedia: Solubility
If you attempt to dissolve 50 g KCl in 100 g water at 50 °C, the resulting mixture is:
Suspension with undissolved solid
Unsaturated clear solution
Supersaturated if shaken
Colloidal dispersion
Since maximum solubility is 45.8 g, attempting to dissolve 50 g leaves 4.2 g undissolved, forming a suspension in equilibrium with the saturated solution. It cannot become supersaturated just by stirring. LibreTexts: Saturated Solutions
How many grams of KCl can dissolve in 250 g water at 50 °C?
114.5 g
45.8 g
250 g
57.3 g
Solubility is 45.8 g per 100 g water, so in 250 g water: (45.8 g/100 g)×250 g=114.5 g. Scaling linear solubility values is standard practice. Chemguide
Which step is essential to prepare a supersaturated KCl solution at 50 °C?
Heat to dissolve more KCl then cool slowly
Add seed crystals before heating
Boil vigorously to remove water
Cool rapidly with stirring
Dissolve excess KCl at an elevated temperature, then cool gently to avoid nucleation. Slow cooling maintains the metastable supersaturated state. Rapid cooling or seeding triggers precipitation. Wikipedia: Supersaturation
What happens to the ionic strength of a solution as KCl solubility increases?
It increases
It decreases
It stays the same
It oscillates
Ionic strength is half the sum of concentration×charge² for all ions. As more K+ and Cl - ions dissolve, their concentrations rise, increasing the ionic strength. Wikipedia: Ionic Strength
What is the molarity of a saturated KCl solution at 50 °C (approximately)?
6.1 M
0.61 M
45.8 M
1.2 M
45.8 g KCl is 0.614 mol in 1 L water approximately. Thus concentration ?0.614 M. However, solution volume increases slightly, giving ~6.1 M if miscalculated by confusion of units - commonly mistaken but correct calculation yields ~0.62 M. LibreTexts: Solubility Product
The metastable zone width for KCl refers to:
Temperature difference between saturation and crystallization
Concentration range of a saturated solution
pH range of solubility
Pressure range of dissolution
Metastable zone width is the temperature interval over which a solution remains supersaturated without crystallization. It quantifies how much below saturation temperature one can cool before spontaneous nucleation. ScienceDirect: Metastable Zone
What percent by mass is KCl in a saturated solution at 50 °C?
31.4%
45.8%
50.0%
20.0%
Mass percent = (mass solute)/(mass solute + mass solvent)×100 = 45.8/(45.8+100)×100 ?31.4%. This metric compares solute fraction in the solution. Wikipedia: Mass Fraction
At saturation, which dynamic process occurs in a KCl solution at 50 °C?
Dissolution rate equals crystallization rate
Only dissolution continues
Only crystallization continues
No molecular exchange
In a saturated solution, dynamic equilibrium is established: solute particles dissolve and precipitate at the same rate, keeping concentration constant. This is a hallmark of chemical equilibria. Wikipedia: Chemical Equilibrium
Which factor does NOT significantly affect KCl solubility at 50 °C?
Stirring rate
Temperature
Presence of common ions
Solvent composition
Stirring accelerates reach of equilibrium but does not change equilibrium solubility. Temperature, common ions, and solvent polarity/composition directly alter solubility limits. LibreTexts: Solutions
Given KCl solubility of 45.8 g per 100 g water at 50 °C, what is its approximate Ksp value (mol²/L²)?
0.38
1.10
0.0458
2.14
45.8 g/100 g water =0.614 mol in ~0.1 L ?6.14 M. Ksp=[K+][Cl - ]=s²?(6.14)²?37.7. However, proper volume correction gives s?0.614 M ?Ksp?(0.614)²?0.38. LibreTexts: Solubility Product
0
{"name":"What is the approximate solubility of KCl in 100 g of water at 50 °C?", "url":"https://www.quiz-maker.com/QPREVIEW","txt":"What is the approximate solubility of KCl in 100 g of water at 50 °C?, How does the solubility of KCl change as temperature increases from 20 °C to 50 °C?, What term describes a solution that contains more dissolved KCl than the saturation point at 50 °C?","img":"https://www.quiz-maker.com/3012/images/ogquiz.png"}

Study Outcomes

  1. Interpret KCl Saturation Data -

    Understand how a solution of KCl is saturated at 50 °C by reading and interpreting solubility values from Table G.

  2. Apply Table G Solubility Levels -

    Use table G solubility levels in solutions to calculate the maximum amount of KCl that dissolves at various temperatures.

  3. Analyze Supersaturated NaNO₃ Behavior -

    Examine a supersaturated solution for NaNO₃ at a temperature of 5 °C to determine stability and potential crystal formation.

  4. Predict Precipitation and Dissolution -

    Predict whether KCl or NaNO₃ will precipitate or dissolve when temperatures change around 50 °C and 5 °C.

  5. Compare Solubility Patterns -

    Contrast the solubility trends of KCl at 50 °C with those of NaNO₃ at 5 °C to draw conclusions about temperature's effect on different salts.

Cheat Sheet

  1. KCl Solubility at 50°C -

    When a solution of kcl is saturated at 50 c, Table G solubility levels in solutions indicate it holds about 45 g of KCl per 100 g of water. This key value, tabulated by the CRC Handbook and verified by the University of Wisconsin, guides stoichiometric calculations in lab prep. Remember: precise mass measurements prevent under- or over-saturation.

  2. Creating Supersaturated NaNO₃ at 50°C -

    A supersaturated solutionn for nano3 at the temprature for 50c is achieved by dissolving excess NaNO₃ (up to ~85 g per 100 g water) at high heat. Rapid heating dissolves more solute, and gentle cooling retains this excess above the equilibrium solubility limit. Use NIST solubility data to track how much extra salt stays dissolved.

  3. Triggering Supersaturation at 5°C -

    By carefully cooling the hot NaNO₃ mixture to create a supersaturated solution for nano3 at a tempature of 5c, you maintain solution stability until disturbed. According to the Journal of Chemical Education, such cooling at controlled rates avoids premature crystallization. A seed crystal or shock will then initiate rapid precipitation.

  4. Interpreting Table G Solubility Curves -

    Table G solubility levels in solutions provide temperature vs. solute graphs for common salts like KCl and NaNO₃, enabling you to interpolate values at non-tabulated temperatures. Use linear interpolation between known points for accuracy, as recommended by the Royal Society of Chemistry. This skill predicts whether adding solute will result in a saturated, unsaturated, or supersaturated system.

  5. Mnemonics for Solubility Trends -

    Remember "Solid Increases with Temperature" (SIT) to recall that most ionic solids like KCl and NaNO₃ dissolve more readily at higher temperatures. This handy phrase is supported by thermodynamic data from MIT's OpenCourseWare, illustrating endothermic dissolution. Such mnemonics boost recall during quizzes and exams.

Make a Quiz (FREE) Copy & Edit This Quiz Create a Quiz with AI

Chemistry Quizzes

Powered by: Quiz Maker