solutions & acid and base review game chemistry. name the acid hbr
TRANSCRIPT
Solutions & Acid and Base Review Game
Chemistry
Name the Acid
HBr
Name the Acid
HBr Hydrobromic Acid
Write the Formula
Lithium hydroxide
Write the Formula
Lithium hydroxide LiOH
Name the Base
Mg(OH)2
Name the Base
Mg(OH)2 Magnesium Hydroxide
Properties
What is the “technical” definition of an acid in regards to ?
Arrhenius
What is the “technical” definition of an acid in regards to ? A substance which contains more H+ than OH-
Write the Formula
Hydroiodidic Acid
Write the Formula
Hydroiodidic Acid HI
Properties
What is the “technical” definition of a base
Arrhenius
What is the “technical” definition of a base? A substance which contains more OH- than H+
Name the Base
KOH
Name the Base
KOH Potassium Hydroxide
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 2.0 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 Acid
H2SO4
Name the Acid
H2SO4 Sulfuric Acid
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
Neutralization Reaction
Write the complete balanced equation for the neutralization of nitric acid with calcium hydroxide
Neutralization Reaction
Write the complete balanced equation for the neutralization of phosphoric acid with calcium hydroxide 2HNO3 + Ca(OH)2 Ca(NO3)2 + 2H2O
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)
What mass 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) M = moles/liters .25 = moles/0.075 n = 0.01875 mol x 249.5 = 4.7 g
Name the Acid
HNO2
Name the Acid
HNO2 Nitrous Acid
How many grams 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 3.50 L of a 1.15 M solution? M = moles/liters 1.15 = moles/3.5 n = 4.025 mol x 342 = 1376.55 g
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 0.15 grams of sodium hydroxide in 4500 mL of water?
NaOH 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
Sulfuric Acid
Write the Formula
Phosphoric Acid H2SO4
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 0.0750 moles of NaHCO3 in a volume of 115 mL M = moles/liters M = 0.075/.115 = 0.65 M
Write the Formula
Nitric Acid
Write the Formula
Nitric Acid HNO3
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 2.00 L of solution, what is its molar concentration? How many moles would there be in 350 mL of solution? M = moles/liters M = 3/2 = 1.5M 1.5 = moles/0.35 moles = 0.53 mol
Write the Formula
Sodium carbonate
Write the Formula
Sodium carbonate Na2CO3
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 0.85 M solution of formic acid HCO2H? M = moles/liters 0.85 = moles/1 moles = 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 5.4 grams of sulfuric acid in 250 mL of water?
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 M = 0.055/0.25 = 0.22 M
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? M = 0.94/0.45 = 2.1 M
Write the Formula
Barium hydroxide
Write the Formula
Barium hydroxide Ba(OH)2
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 0.50M NaOH must be added to titrate 46 mL of 0.40 M HClO4
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
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? Molarity of Acid = [H+] 10-2.65
= 0.0022M
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 27.4 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 3.8M 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 3.8M 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. What is the new concentration of the NaCl?
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. 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. 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
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. What is the volume of the solution? 50 g K2CrO4 / 194 = 0.26 mol 1.4 = .26/liters V = 0.184 L
Write the Formula
Acetic Acid
Write the Formula
Acetic Acid HC2H3O2
Name the Acid
HCl
Name the Acid
HCl Hydrochloric Acid
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 3.25 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