Chemistry Chapters 8/9 Flashcards
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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?

<p>A heterogeneous mixture.</p> 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.

<p>Homogeneous mixture (colloid)</p> 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.

<p>Electrolyte</p> 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?

<p>6.4 eq</p> 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?

<p>123 mEq</p> 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?

<p>22 mEq</p> Signup and view all the answers

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

<p>Yes</p> 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?

<p>No</p> Signup and view all the answers

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

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

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

<p>Increase in solubility</p> Signup and view all the answers

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

<p>Increase in solubility</p> 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.

<p>14%, 0.70%</p> 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?

<p>81%</p> 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?

<p>2.3 g NaCl</p> 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?

<p>3M</p> 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?

<p>83 mL</p> 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.

<p>7.3 g</p> 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?

<p>0.4 M</p> 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?

<p>5 mL</p> Signup and view all the answers

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

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

A _____ has lower osmotic pressure than body fluids.

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

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

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

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

<p>177 g</p> 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?

<p>29.5%</p> Signup and view all the answers

What is the formula for volume/volume?

<p>Volume of ethanol (solute) x 100 / (solute + solvent)</p> 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?

<p>0.638 M</p> 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

<p>(NH4)2SO4</p> Signup and view all the answers

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

<p>An ion-dipole interaction</p> Signup and view all the answers

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

<p>Na3PO4</p> Signup and view all the answers

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

<p>1.6 x 10^-8</p> 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)

<p>CO2(g) + H2O(l) + 2 NaCH3COO(aq)</p> 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)

<p>HSO4-</p> Signup and view all the answers

What is an Arrhenius Acid?

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

What is an Arrhenius Base?

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

What is a Bronsted Lowry acid?

<p>Proton (H+) donor.</p> Signup and view all the answers

What is a Bronsted Lowry base?

<p>Proton (H+) acceptor.</p> Signup and view all the answers

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

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

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

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

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

<p>OH-</p> Signup and view all the answers

What are examples of strong acids?

<p>HI, HBr, HCl, H2SO4, HNO3</p> Signup and view all the answers

What are some examples of weak acids?

<p>H3PO4, HF, H2CO3, HCN</p> Signup and view all the answers

What are common strong bases?

<p>LiOH, NaOH, KOH, C5OH</p> Signup and view all the answers

In terms of equilibrium, ____ always points to the ____.

<p>Stronger always points to the weaker.</p> 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

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

Kw = ?

<p>[H3O+] + [OH-]</p> 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?

<p>2.5 x 10^-7, basic</p> Signup and view all the answers

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

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

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

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

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

<p>1 x 10^-12</p> 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.

<p>6.67 x 10^-15</p> Signup and view all the answers

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

<p>0.01</p> Signup and view all the answers

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

<p>1.58 x 10^-6 or 0.00000158</p> Signup and view all the answers

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

<p>H+ + OH- ----&gt; H2O</p> Signup and view all the answers

For a salt: MA

<p>M= base, A= acid</p> 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?

<p>0.111 M HCl</p> 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

<p>4.74</p> 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.

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