UNITS 9 & 10 Review Game Chemistry

Write the Formula Lithium hydroxide

Write the Formula Lithium hydroxide LiOH

Name the Acid HBr

Name the Acid HBr Hydrobromic Acid

If a soap has a hydrogen ion concentration of 2 If a soap has a hydrogen ion concentration of 2.0 x 10-6 M, what is the pH of the solution? Is it an acid or a base?

If a soap has a hydrogen ion concentration of 2 If a soap has a hydrogen ion concentration of 2.0 x 10-6 M, what is the pH of the solution? Is it an acid or a base? [H+] = 2 x 10-6M pH = -log(2 x 10-6) = 5.7 Acid because pH < 7

What is the hydroxide ion concentration of a solution with a pH of 2.3? Is the substance an acid or base?

What is the hydroxide ion concentration of a solution with a pH of 2.3? Is the substance an acid or base? pOH = 14 – 2.3 = 11.7 [OH-] = 10-11.7 = 2 x 10-12 M Acid because pH < 7

Name the Base Mg(OH)2

Name the Base Mg(OH)2 Magnesium Hydroxide

Write the Formula Hydroiodidic Acid

Write the Formula Hydroiodidic Acid HI

I used 50 grams of potassium chromate to make a 1. 4M solution I used 50 grams of potassium chromate to make a 1.4M solution. What is the volume of the solution?

I used 50 grams of potassium chromate to make a 1. 4M solution I used 50 grams of potassium chromate to make a 1.4M solution. What is the volume of the solution? 50 g K2CrO4 / 194 = 0.26 mol 1.4 = .26/v V = 0.184 L

What is the molarity of a potassium hydroxide solution which contains 0.94 moles of potassium hydroxide in 450 mL of water?

What is the molarity of a potassium hydroxide solution which contains 0.94 moles of potassium hydroxide in 450 mL of water? CM = 0.94/0.45 = 2.1 M

Name the Acid H2SO4

Name the Acid H2SO4 Sulfuric Acid

Name the Base KOH

Name the Base KOH Potassium Hydroxide

What is the hydrogen ion concentration of a sample of phosphoric acid that has a pH of 4.9?

What is the hydrogen ion concentration of a sample of phosphoric acid that has a pH of 4.9? [H+] = 10-4.9 = 1.3 x 10-5M

Neutralization Reaction Write the balanced neutralization reaction for nitrous acid reacting with potassium hydroxide?

Neutralization Reaction Write the balanced neutralization reaction for nitrous acid reacting with potassium hydroxide? HNO2 + KOH  KNO2 + H2O

Name the Base Ca(OH)2

Name the Base Ca(OH)2 Calcium Hydroxide

Name the Acid HNO2

Name the Acid HNO2 Nitrous Acid

Neutralization Reaction Write the complete balanced equation for the neutralization of phosphoric acid with calcium hydroxide

Neutralization Reaction Write the complete balanced equation for the neutralization of phosphoric acid with calcium hydroxide 2H3PO4 + 3Ca(OH)2  Ca3(PO4)2 + 6H2O

How many grams of copper (II) sulfate pentahydrate will be needed to make 75 mL of a 0.250 M solution? (The molar mass of copper (II) sulfate pentahydrate is 249.5 g/mole)

How many grams of copper (II) sulfate pentahydrate will be needed to make 75 mL of a 0.250 M solution? (The molar mass of copper (II) sulfate pentahydrate is 249.5 g/mole) CM = n/V .25 = n/0.075 n = 0.01875 mol x 249.5 = 4.7 g

How many kilograms of sucrose, C12H22O11 ,will be needed to make 3 How many kilograms of sucrose, C12H22O11 ,will be needed to make 3.50 L of a 1.15 M solution?

How many kilograms of sucrose, C12H22O11 ,will be needed to make 3 How many kilograms of sucrose, C12H22O11 ,will be needed to make 3.50 L of a 1.15 M solution? CM = n/v 1.15 = n/3.5 n = 4.025 mol x 342 = 1376.55 g / 1000 = 1.38 kg

What is the pH of a solution made with 0 What is the pH of a solution made with 0.15 grams of sodium hydroxide in 4500 mL of water?

What is the pH of a solution made with 0 What is the pH of a solution made with 0.15 grams of sodium hydroxide in 4500 mL of water? 0.15 g / 40 = 0.00375 moles M = 0.00375/4.5 = 8.33X10-4 [OH-] pOH = -log (8.33x10-4) pOH = 3.08 pH = 14-3.08 = 10.92

Write the Formula Phosphoric Acid

Write the Formula Phosphoric Acid H3PO4

Write the Formula Nitric Acid

Write the Formula Nitric Acid HNO3

What is the molarity of a solution that contains 0 What is the molarity of a solution that contains 0.0750 moles of NaHCO3 in a volume of 115 mL

What is the molarity of a solution that contains 0 What is the molarity of a solution that contains 0.0750 moles of NaHCO3 in a volume of 115 mL CM = n/v CM = 0.075/.115 = 0.65 M

A solution has 3. 00 moles of solute in 2 A solution has 3.00 moles of solute in 2.00 L of solution, what is its molar concentration? How many moles would there be in 350 mL of solution?

A solution has 3. 00 moles of solute in 2 A solution has 3.00 moles of solute in 2.00 L of solution, what is its molar concentration? How many moles would there be in 350 mL of solution? CM = n/V CM = 3/2 = 1.5M 1.5 = n/0.35 n = 0.53 mol

Write the Formula Sodium carbonate

Write the Formula Sodium carbonate Na2CO3

Write the Formula Barium hydroxide

Write the Formula Barium hydroxide Ba(OH)2

Describe how you would prepare 1. 00L of a 0 Describe how you would prepare 1.00L of a 0.85 M solution of formic acid HCO2H?

Describe how you would prepare 1. 00L of a 0 Describe how you would prepare 1.00L of a 0.85 M solution of formic acid HCO2H? CM = n/v 0.85 = n/1 n = 0.85 mol x 46 = 39.1 g Take 39.1 grams of formic acid and dissolve in a little bit of water. Put into a 1.00 L volumetric flask and fill to the line with water

What is the molarity of a sulfuric acid solution which contains 5 What is the molarity of a sulfuric acid solution which contains 5.4 grams of sulfuric acid in 250 mL of water?

What is the molarity of a sulfuric acid solution which contains 5 What is the molarity of a sulfuric acid solution which contains 5.4 grams of sulfuric acid in 250 mL of water? 5.4g/98 = 0.055 mol CM = 0.055/0.25 = 0.22 M

In the titration of 35 mL of liquid drain cleaner containing NaOH, 50 mL of 0.4M HCl must be added to reach the equivalence point. What is the molarity of the base in the cleaner?

In the titration of 35 mL of liquid drain cleaner containing NaOH, 50 mL of 0.4M HCl must be added to reach the equivalence point. What is the molarity of the base in the cleaner? MaVa = MbVb (0.4)(50) = Mb(35) 0.57 M

Calculate how many milliliters of 0 Calculate how many milliliters of 0.50M NaOH must be added to titrate 46 mL of 0.40 M HClO4

Calculate how many milliliters of 0 Calculate how many milliliters of 0.50M NaOH must be added to titrate 46 mL of 0.40 M HClO4 MaVa = MbVb 0.4(46) = 0.5Vb Vb = 36.8 mL

Name the Base NaOH

Name the Base NaOH Sodium Hydroxide

Write the Formula Acetic Acid

Write the Formula Acetic Acid HC2H3O2

A 15.5 mL sample of 0.215 M KOH was titrated with an acetic acid solution, It took 21.2 mL of the acid to reach the equivalence point. What is the molarity of the acetic acid?

A 15.5 mL sample of 0.215 M KOH was titrated with an acetic acid solution, It took 21.2 mL of the acid to reach the equivalence point. What is the molarity of the acetic acid? (0.215)(15.5) = Ma(21.2) 0.157 M

What is the molarity of a solution of acetic acid with a pH of 2.65?

What is the molarity of a solution of acetic acid with a pH of 2.65?

A 20 mL sample of an HCl solution was titrated with 27 A 20 mL sample of an HCl solution was titrated with 27.4 mL of a standard solution of NaOH. The concentration of the standard is 0.0154 M. What is the molarity of the HCl?

A 20 mL sample of an HCl solution was titrated with 27 A 20 mL sample of an HCl solution was titrated with 27.4 mL of a standard solution of NaOH. The concentration of the standard is 0.0154 M. What is the molarity of the HCl? (0.0154)(27.4) = Ma(20) = 0.021 M

I want to dilute 20 mL of a 6M solution of acetic acid to a 3 I want to dilute 20 mL of a 6M solution of acetic acid to a 3.8M solution of acetic acid. How much water should I add to the 6M acetic acid to achieve this?

I want to dilute 20 mL of a 6M solution of acetic acid to a 3 I want to dilute 20 mL of a 6M solution of acetic acid to a 3.8M solution of acetic acid. How much water should I add to the 6M acetic acid to achieve this? 6(20) = 3.8V V = 31.6 mL ADD 11.6 mL of water

I mix 20 mL of 4. 5M NaCl with 40 mL of water I mix 20 mL of 4.5M NaCl with 40 mL of water. What is the new concentration of the NaCl?

I mix 20 mL of 4. 5M NaCl with 40 mL of water I mix 20 mL of 4.5M NaCl with 40 mL of water. What is the new concentration of the NaCl? 4.5(20) = M(60) Note: final volume is 20+40 mL water added M = 1.5 M

A 450 mL solution of 1. 5 M HCl is sat out over night A 450 mL solution of 1.5 M HCl is sat out over night. 150 mL of the water evaporated. What is the new concentration of the HCl?

A 450 mL solution of 1. 5 M HCl is sat out over night A 450 mL solution of 1.5 M HCl is sat out over night. 150 mL of the water evaporated. What is the new concentration of the HCl? 1.5 (450) = M (300) NOTE: final vol is 450 – 150 evaporated = 300 2.25 M

What does the term “strong acid” mean?

What does the term “strong acid” mean? Strong acid means that the acid dissociates completely in water

Name the Acid HCl

Name the Acid HCl Hydrochloric Acid

What is the pH of a solution made by putting 6 What is the pH of a solution made by putting 6.0 grams of phosphoric acid in 250 L of water?

What is the pH of a solution made by putting 6 What is the pH of a solution made by putting 6.0 grams of phosphoric acid in 250 L of water? 6 g H3PO4 / 98 = 0.0612 mol [H3PO4] = 0.0612 / 250 = 2.45 x 10-4 [H+] = 3(2.45 x 10-4) = 7.35 x 10-4 pH = -log(7.35 x 10-4) = 3.13

What is the pH of a solution made by putting 3 What is the pH of a solution made by putting 3.25 grams of strontium hydroxide in 5000 L of water?

What is the pH of a solution made by putting 3 What is the pH of a solution made by putting 3.25 grams of strontium hydroxide in 5000 L of water? 3.25 g Sr(OH)2 / 121.6 = 0.0267 mol [Sr(OH)2] = 0.0267/ 5000 = 5.34 x 10-6M [OH-] = 2(5.34 x 10-6) = 1.07 x 10-5 M pOH = -log(1.07 x 10-5) = 4.97 pH = 14 – 4.97 = 9.03