chem

What is the molarity of a KCl solution made by diluting 75.0 mL of a 0.200 M solution to a final volume of 100. mL?

0.150 M

35.0 mL of a 0.320 M NaBr solution is diluted to 65.0 mL

0.172 M

What volume of 0.10 M NaOH can be prepared from 250. mL of 0.30 M NaOH?

0.75 L

How many moles of CaCl2 are in 250 mL of a 3.0 M of CaCl2 solution?

0.75 mole

75.0 mL of a 4.40 M NaOH solution is diluted to 305 mL

1.08 M

You need 500. mL of a 4.5 % (m/v) glucose solution. If you have a 22 % (m/v) glucose solution on hand, how many milliliters of this solution do you need?

100 mL

If there are 740 mL of champagne in the bottle, how many milliliters of alcohol are present?

110 ml

A solution contains 0.254 moles of NaCl in 250. g of water. How many grams of solute are present and what is the mass percent (m/m)?

14.8 g, 5.92%

What is the molarity of a solution that contains 17 g of NH3 in 0.50 L of solution?

2.0 M

What is the concentration, mass/volume percent (m/v), of a solution prepared from 50. g NaCl and 2.5 L of water?

2.0% (m/v)

What is the new mass/volume percent (m/v) of a KOH solution that is prepared by diluting 110 mL of a 6.0% (m/v) KOH solution to 330 mL?

2.0% (m/v)

What is the molarity of a solution containing 5.0 moles of KCl in 2.0 L of solution?

2.5 M

What is the concentration, in mass percent (m/m), of a solution prepared from 50.0 g NaCl and 150.0 g of water?

25.0% (m/m)

What is the overall balanced equation for the precipitation reaction occurring between silver nitrate and calcium bromide?

2AgNO3(aq)+CaBr2(aq)→2AgBr(s)+Ca(NO3)2(aq)

Rubbing alcohol is 70.% (v/v) isopropyl alcohol by volume. How many mL of isopropyl alcohol are in a 1 pint (473 mL) container?

330 mL

200. mL of a 12.0% (m/v) NaCl solution is diluted to 600. mL. The new concentration is ________ %.

4.00 % (m/v)

21.0 mL of a 15.0 %(m/v) K2SO4 solution is diluted to 72.0 mL

4.38 %(m/v)

5.0 g of casein in 110 mL of low-fat milk

4.5 %

Calculate the mass percent (m/m) of a solution containing 39 g of K2CO3 and 714 g of H2O.

5.2 % (m/m)

A solution which has 12 g of solute dissolved in 200.mL of solution has a m/v concentration of ________.

6.0 % m/v

A 2.0% (m/v) NaCl solution contains ________ g NaCl in 300. mL of solution.

6.0 g

A red blood cell will undergo crenation in ________.

7% NaCl

6.00 g of LiCl in 77.0 mL of LiCl solution

7.79 %

How many grams of glucose are needed to prepare 400. mL of a 2.0%(m/v) glucose solution?

8.0 g

30.0 mL of acetic acid and 300. mL of water

Acetic acid is the solute, water is the solvent.

1.0 g of Br2 and 50.0 mL of methylene chloride(l)

Bromine is the solute, methylene chloride is the solvent.

What precipitate will form when aqueous solutions of sodium carbonate (Na2CO3) and calcium chloride (CaCl2) are mixed?

CaCO3(s)

A 44.0 −mL sample of a 10 % (m/v) H2SO4 solution is added to water to give a final volume of 410 mL .

Cfinal = 1.1 % (m/v)

Water is added to 0.40 L of a 14 M NaOH solution to make 5.0 L of a diluted NaOH solution

Cfinal = 1.1 M

3.0 L of a 4.0 M HCl solution is added to water so that the final volume is 6.0 L .

Cfinal = 2.0 M

A 15.0 −mL sample of a 25 % (m/v) KOH solution is diluted with water so that the final volume is 100.0 mL .

Cfinal = 3.8 % (m/v)

The_________ completely dissociates into_________when it dissolves in water. When the_______dissolves in water, there are a few_______present, but mostly__________.

Strong electrolyte KF, K+ and F- ions, weak electrolyte HF, H+ and F- ions, HF molecules

100.0 mL of water and 4.0 g of sugar

Sugar is the solute, water is the solvent.

A solution is a homogenous mixture of solute and solvent. There are different types of solutions. A carbonated drink is an example of a solution where the solute is a gas and the solvent is a liquid. Sugar crystals dissolved in water is an example of a solution where the solute is a solid and the solvent is liquid. Acetic acid is miscible in water, forming a solution commonly known as vinegar. In this case, both the solute and the solvent are liquids. The solubility of solute in a solvent depends on various parameters, such as temperature, pressure, the nature of the solute, and the nature of the solvent. Considering these parameters, identify the statements that are correct for the solubility of a solute in a solvent.

Table salt dissolves in water to form a solution. Zinc sulfate is soluble in water. Carbon dioxide gas will be less soluble in water when the partial pressure is low.

Identify which statement about a solution is correct.

The solution has the same physical state as the physical state of the solvent.

urea solution

Urea will be found outside the bag in the distilled water.

How many milliliters of alcohol are present in 800 mL of brandy?

Valcohol = 320 mL

KCl solution and glucose solutions

potassium ions, chloride ions, and glucose molecules

an albumin solution (colloid), KCl solution, and glucose solution

potassium ions, chloride ions, and glucose molecules

When some of the sugar added to iced tea remains undissolved at the bottom of the glass, the solution is ________.

saturated

adding 19 g of KNO3 to 50. g of H2O

saturated

adding 68 g of KNO3 to 150. g of H2O

saturated

urea solution and NaCl solution

sodium ions, chloride ions, and urea molecules

(NH4)2SO4

soluble

NaHCO3

soluble

K2SO4

soluble in water

LiCl

soluble in water

Na2S

soluble in water

A mixture is prepared by dissolving 2 g of KCl in 100 g of H2O. In this mixture, H2O is the ________.

solvent

In the process known as osmosis, ________ moves through a semipermeable membrane into an area of ________ concentration.

solvent, lower solvent

When KCl dissolves in water ________.

the K+ ions are attracted to the partial negative charge on the oxygen atom of the water molecule

adding 32 g of KNO3 to 200. g of H2O

unsaturated

A red blood cell will undergo hemolysis in ________.

water

The rate at which a solute dissolves in a solvent depends on the kinetic energy of the solution, the time of contact, and the surface area of contact between the solute and the solvent particles. Both endothermic and exothermic dissolution processes will respond similarly to each factor, however the change may be more pronounced depending on the thermodynamic parameters of the reaction. As the kinetic energy, time of contact, and surface area of contact between the solute and the solvent particles increase, the rate at which the solute undergoes dissolution in a solvent increases. Similarly, as the kinetic energy, time of contact, and surface area of contact between the solute and the solvent particles decrease, the rate at which the solute undergoes dissolution in a solvent decreases. The dissolution process can be altered by varying these parameters, such as by increasing or decreasing the temperature or by reducing the particle size of the solute. Consider the preparation of a NaCl salt solution using coarse crystals of NaCl in an unstirred container at room temperature. Classify the following conditions based on the change in the rate of dissolution of NaCl in water compared to the initial preparation if the dissolution process is endothermic.

Faster Dissolution process: NaCl salt is added to water, and the mixture is stirred. NaCl salt is added to water, and the mixture is heated. Finely powdered NaCl salt is added to water. Slower dissolution Process: A large piece of NaCl salt is added to water. NaCl salt is added to water, and the mixture is cooled.

FePO4

Insoluble in water

The ______ at the surface of the solid are pulled into solution by the_______ water molecules, where the________ process surrounds separate_______ with water molecules.

K+ and I− ions, polar, hydration, ions

LiI solution

Li+ and I− ions will be found outside the bag in the distilled water.

5.75 g of NaCl in 400. mL of a NaCl solution

Molarity = 0.246 M

What is the molarity of a solution containing 6.5 g of NaOH in 500. mL of NaOH solution?

Molarity = 0.33 M

5.00 moles of glucose in 3.50 L of a glucose solution

Molarity = 1.43 M

6.00 g of KOH in 3.00 L of a KOH solution

Molarity = 3.56×10−2 M

Consider the following ionic compounds: CdCO3, Na2S, PbSO4, (NH4)3PO4, and Hg2Cl2. Which compounds will be soluble when added to water?

Na2S and (NH4)3PO4

When sodium chloride, NaCl, is added to water, it forms a solution. The steps involved in the dissolution of NaCl in water are shown below. Sodium Ions, Chloride ions, water molecules Order the steps involved in the formation of a solution.

NaCL crystal is added to water Na+ ions are attracted to H2O and Cl- ions are attracted to H2O NaCl solution

Predict the products for the following precipitation reaction: NiCl2(aq)+(NH4)2S(aq)→

NiS(s)+2NH4Cl(aq)

KCl solution and starch solution (colloid)

Only K+ and Cl− ions will be found outside the bag in the distilled water.

starch solution (colloid) and histidine, an amino acid, solution

Only histidine will be found outside the bag in the distilled water

Water is a polar solvent and hexane (C6H14) is a nonpolar solvent. In which solvent is each of the following, which is found or used in the body, more likely to be soluble?

Soluble in Water: riboflavin (vitamin B2), polar and FeSO4 (iron supplement), ionic Soluble is hexane: oleic acid (lipid), nonpolar and canola oil, nonpolar

The solubility of KI is 50 g in 100 g of H2O at 20 °C. If 110 grams of KI are added to 200 grams of H2O, ________.

a saturated solution will form

Water is considered a polar solvent due to attractive forces known as hydrogens bonds. A hydrogen bond is _______________________.

an attractive force between molecules where partially positive hydrogen atoms are attracted to partially negative atoms of F, O, or N.

The strong electrolyte NaOH will________ when placed in water. It will form ________ after it is mixed in water. However, the nonelectrolyte CH3OH will_________ when placed in water and will form _________ in the water.

dissociate completely, Na_ and OH- ions, remain as molecules, CH3OH molecules

an albumin solution (colloid)

distilled water only

A substance that carries an electric current when dissolved in water is called a(n) ________.

electrolyte

15% (m/v) glucose

hypertonic

1 % (m/v) glucose

hypotonic

A solution that has an osmotic pressure less than that of red blood cells is called ________.

hypotonic

distilled H2O

hypotonic

According to Henry's law, the solubility of a gas in a liquid ________.

increases as the gas pressure above the liquid increase

An increase in the temperature of a solution usually ________.

increases the solubility of a solid solute in the solution

Ag2O

insoluble

Ag2S

insoluble

CaCO3

insoluble

CuCO3

insoluble

Mg3(PO4)2

insoluble

Mg3(PO4)2 soluble or insoluble?

insoluble

Pb(OH)2

insoluble

PbF2

insoluble

PbS

insoluble in water

0.9% (m/v) NaCl

isotonic

A solution with the same osmotic pressure as the blood is ________.

isotonic to the blood

Calculate the mass percent of a solution containing 10.5 g of Na2SO4 and 75.5 g of H2O.

mass percent = 12.2 %(m/m)

The molarity (M) of a solution refers to ________.

moles of solute/L of solution

does not dissolve in water because ________.

oil is nonpolar