Chemistry Chapters 8/9 Flashcards

Questions and Answers

What is the solute?

The lesser of the substances, the thing being dissolved.

What is a solvent?

The greater of the substances, the thing doing the dissolving.

What is a colloid?

A homogeneous mixture with an opaque appearance.

What is a Suspension?

A heterogeneous mixture. Signup and view all the answers

Classify each as a heterogeneous mixture (suspension), a homogeneous mixture (colloid), or a solution: chocolate chip ice cream, mayonnaise, nail polish remover, brass.

Homogeneous mixture (colloid) Signup and view all the answers

Classify each solution as an electrolyte or nonelectrolyte: a.KCL in H2O, b.Sucrose (C12H22O11) in H2O, c.KI in H2O.

Electrolyte Signup and view all the answers

How many equivalents of sulfate ions are present in a solution that contains 3.2 moles of sulfate ions?

6.4 eq Signup and view all the answers

If an intravenous aqueous NaCl solution contains 154 mEq/L of Na+ ions, how many miliequivalents of Na+ is a patient given in 800 mL of solution?

123 mEq Signup and view all the answers

A KCL given to a patient contains 40 mEq of K+ per liter, how many miliequivalents of K+ are present in 550 mL of the solution?

22 mEq Signup and view all the answers

Predict the water solubility of each compound: KCL, CH3OH, C6H14.

Yes Signup and view all the answers

Which pairs of compounds will form a solution: a) C6H6 and C6H14, b) Na2SO4 and H2O, c) NaCl and C6H14, d) H2O and CCl4?

No Signup and view all the answers

Predict whether the following ionic compounds are soluble in water: a) Na3PO4, b) Mg3(PO4)2, c) KOH.

Yes Signup and view all the answers

For solids, what causes solubility to change: a) increasing temp, b) increasing pressure?

Increase in solubility Signup and view all the answers

For gases, what causes solubility to change: a) increasing temp, b) increasing pressure?

Increase in solubility Signup and view all the answers

Calculate the weight/volume percent concentration of each component in a commercial mouthwash that contains 4.3 g of ethanol and 0.21 g of antiseptic in each 30 mL portion.

14%, 0.70% Signup and view all the answers

What is the volume/volume percent concentration of ethanol in a 1 oz bottle that contains 24 mL of ethanol?

81% Signup and view all the answers

How many grams of NaCl are contained in 250 mL of a saline solution that contains 0.92% w/v NaCl in water?

2.3 g NaCl Signup and view all the answers

What is the molarity of an intravenous glucose solution prepared from 108 g of glucose in 2.0 L of solution?

3M Signup and view all the answers

What is the volume in mL of a 0.30 M solution of glucose that contains 0.025 mol of glucose?

83 mL Signup and view all the answers

How many grams of NaCl are contained in each of the following volumes of 1.25 M solution: a) 10 L, b) 55 L.

7.3 g Signup and view all the answers

What is the concentration of a solution formed by diluting 5.0 mL of a 3.2 M glucose solution to 40.0 mL?

0.4 M Signup and view all the answers

How many mL of a 4.0% (w/v) solution must be used to prepare 250 mL of a 0.80% (w/v) solution?

5 mL Signup and view all the answers

What do you call two solutions with the same osmotic pressure?

Isotonic Signup and view all the answers

A _____ has lower osmotic pressure than body fluids.

Hypotonic Signup and view all the answers

A _____ solution has a higher osmotic pressure than body fluids.

Hypertonic Signup and view all the answers

How many grams of glucose (C6H12O6) are contained in 555 mL of a 1.77 M glucose solution?

177 g Signup and view all the answers

A solution is made by mixing 569 mL of water and 238 mL of ethanol. What is the concentration of ethanol in units of volume/volume percent?

29.5% Signup and view all the answers

What is the formula for volume/volume?

Volume of ethanol (solute) x 100 / (solute + solvent) Signup and view all the answers

What is the molarity of a 11.5% (w/v) glucose (C6H12O6, molar mass 180.16 g/mol) solution?

0.638 M Signup and view all the answers

Which ionic compound is not soluble in water? A) NaCl B) AgCl C) Ca(CH3CO2)2 D) (NH4)2SO4

(NH4)2SO4 Signup and view all the answers

The attraction of an ion with a dipole in a molecule is called?

An ion-dipole interaction Signup and view all the answers

Which salt forms a basic solution when dissolved in water? A) NH4Br B) KCl C) LiNO3 D) Na3PO4

Na3PO4 Signup and view all the answers

What is the [H3O+] concentration in egg whites if the [-OH] is 6.3 × 10^-7 M?

1.6 x 10^-8 Signup and view all the answers

What are the products of the acid-base reaction of sodium carbonate with acetic acid? A) H2CO3(aq) + H2O(l) + 2 NaOH(aq) B) CO2(g) + H2O(l) + 2 NaCH3COO(aq) C) 5 CO2(g) + 2 H2O(l) + 2 NaOH(aq) D) CO(g) + H2O(l) + 2 NaCH3COO(aq)

CO2(g) + H2O(l) + 2 NaCH3COO(aq) Signup and view all the answers

Which acid is the strongest? a) Ammonium ion NH4+ (Ka = 5.6 × 10^-10) b) Hydrogen sulfate ion HSO4- (Ka = 1.2 × 10^-2) c) Hydrofluoric acid HF (Ka = 7.2 × 10^-4) d) Hydrocyanic acid HCN (Ka = 4.9 × 10^-10)

HSO4- Signup and view all the answers

What is an Arrhenius Acid?

Contains a hydrogen atom and dissolves in H2O to form a hydrogen ion. Signup and view all the answers

What is an Arrhenius Base?

Contains a hydroxide and dissolves in H2O to form OH- Signup and view all the answers

What is a Bronsted Lowry acid?

Proton (H+) donor. Signup and view all the answers

What is a Bronsted Lowry base?

Proton (H+) acceptor. Signup and view all the answers

The one with more H+ is always the...?

Acid Signup and view all the answers

Determine the conjugate acid of each base: a) F-, b) NO3-, c) H2O.

HF Signup and view all the answers

Determine the conjugate base of each acid: a) H2O, b) HCO3-, c) H2S.

OH- Signup and view all the answers

What are examples of strong acids?

HI, HBr, HCl, H2SO4, HNO3 Signup and view all the answers

What are some examples of weak acids?

H3PO4, HF, H2CO3, HCN Signup and view all the answers

What are common strong bases?

LiOH, NaOH, KOH, C5OH Signup and view all the answers

In terms of equilibrium, always points to the .

Stronger always points to the weaker. Signup and view all the answers

Are the reactants or products favored at equilibrium in each reaction? a) HF + OH ----> F + H2O b) NH4 + Cl -----> NH3 + HCl

Reactants Signup and view all the answers

Kw = ?

[H3O+] + [OH-] Signup and view all the answers

If the H3O in blood is 4.0 x 10^-6 M, what is the value of OH-? Is blood acidic, basic, or neutral?

2.5 x 10^-7, basic Signup and view all the answers

If H3O > 10^-7, what does this imply?

Acidic Signup and view all the answers

If OH > 10^-7, what does this imply?

Basic Signup and view all the answers

Calculate the values of H3O and OH in a 0.01 M NaOH solution.

1 x 10^-12 Signup and view all the answers

Calculate the values of H3O and OH in each solution: a) 0.001, b) 1.5 M, c) 30 M.

6.67 x 10^-15 Signup and view all the answers

What is the H3O concentration in lemon juice that has a pH of about 2?

0.01 Signup and view all the answers

What is the H3O concentration in sweat that has a pH of 5.8?

1.58 x 10^-6 or 0.00000158 Signup and view all the answers

Write the net ionic equation for hydrochloric acid and sodium hydroxide.

H+ + OH- ----> H2O Signup and view all the answers

For a salt: MA

M= base, A= acid Signup and view all the answers

What is the molarity of an HCl solution if 22.5 mL of a 0.100 M NaOH solution is needed to titrate a 25.0 mL sample of the acid?

0.111 M HCl Signup and view all the answers

What is the pH of a buffer that contains a 0.20 M CH3COOH and a 0.20 M NaCH3COO? Ka= 1.8 x 10^-5

4.74 Signup and view all the answers

Study Notes

Solutions and Mixtures

Solute: The substance that is dissolved in a solution; present in lesser amount.
Solvent: The medium doing the dissolving; present in greater amount.
Colloid: A homogeneous mixture with an opaque appearance, examples include milk, mayonnaise, and Jello-O.
Suspension: A heterogeneous mixture where particles are not uniformly distributed, examples include mud and chalk water.

Mixture Classifications

Heterogeneous Mixtures (Suspensions): Examples include chocolate chip ice cream and mud.
Homogeneous Mixtures (Colloids): Examples include mayonnaise.
Solutions: Examples include nail polish remover and brass.

Electrolytes vs Non-electrolytes

Electrolytes: Conduct electricity when dissolved in water; examples include KCl and KI.
Non-electrolytes: Do not conduct electricity when dissolved; sucrose is an example.

Ion Equivalents

Sulfate Ions: 3.2 moles of sulfate ions correspond to 6.4 equivalents.
Intravenous NaCl Solution: Contains 154 mEq/L of Na+ ions; 800 mL gives a total of 123 mEq.
KCl Solution: Contains 40 mEq of K+ per liter; 550 mL yields 22 mEq.

Solubility Forecasts

Soluble Compounds in Water: KCl, CH3OH, and KOH are generally soluble; C6H14 is not.
Ionic Compounds: Na3PO4 is soluble, Mg3(PO4)2 is not, and KOH is soluble.

Influence of Temperature and Pressure

Solubility of Solids: Increasing temperature leads to increased solubility; increasing pressure has no effect.
Solubility of Gases: Increasing temperature leads to decreased solubility; increasing pressure increases solubility.

Concentration Calculations

Weight/Volume Percent Concentration: Example for mouthwash: 4.3 g ethanol and 0.21 g antiseptic in 30 mL yields 14% and 0.70%.
Volume/Volume Percent Concentration: Example: 24 mL of ethanol in 1 oz bottle (29.57 mL) yields 81%.
Molarity Calculation: 108 g of glucose in 2.0 L results in 0.3 M.
W/V for NaCl: A 0.92% w/v NaCl solution in 250 mL contains 2.3 g NaCl.

Osmotic Pressure

Isotonic Solutions: Solutions with equal osmotic pressure.
Hypotonic Solutions: Have lower osmotic pressure than body fluids.
Hypertonic Solutions: Have higher osmotic pressure.

Glucose Solutions

Molarity of Glucose: A 1.77 M glucose solution in 555 mL contains 177 g of glucose.
Volume Percent of Ethanol: Mixing 569 mL of water with 238 mL of ethanol yields a 29.5% concentration.
Dilution Calculation: Diluting a 5.0 mL of 3.2 M glucose solution to 40.0 mL results in 0.4 M.

Acid-Base Reactions

Arrhenius Acids and Bases: Acids contain H+ ions (e.g., HCl); bases contain OH- ions (e.g., NaOH).
Bronsted-Lowry Definitions: Acids are proton donors; bases are proton acceptors.
Conjugate Pairs: The conjugate acid of F- is HF, and the conjugate base of H2O is OH-.

Acid Strength and Equilibrium

Strong Acids: Include HI, HBr, HCl, H2SO4, HNO3; weaker acids include H3PO4 and H2CO3.
Osmotic Equilibrium: At equilibrium, the reaction favors the side with the weaker acid or base.

Ionic Equations and pH Calculations

Net Ionic Reaction: H+ + OH- → H2O for HCl and NaOH.
H3O Concentration: Lemon juice with pH 2 has an H3O concentration of 0.01 M.
Buffer pH Calculation: For 0.20 M CH3COOH and NaCH3COO, pH calculates to 4.74.

Important Constants

Kw (Ion Product of Water): Kw = [H3O+][OH-].

Chemical Properties in Solutions

A solution with H3O+ > 10-7 M is acidic; if OH- > 10-7 M, it is basic.
A 0.01 M NaOH solution yields H3O and OH values, demonstrating acid-base dynamics and equilibrium behavior.

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Test your knowledge on the concepts of solutes, solvents, colloids, and suspensions with these flashcards covering Chapters 8 and 9 of chemistry. Understand the definitions and examples to enhance your grasp of mixtures and their characteristics.