Chemistry Test 4
When some of the sugar added to iced tea remains undissolved at the bottom of the glass, the solution is When some of the sugar added to iced tea remains undissolved at the bottom of the glass, the solution is dilute. saturated. polar. nonpolar. unsaturated.
saturated
a mixture that cannot be separated by a semipermeable membrane characteristic of a suspension characteristic of a solution characteristic of a colloid
solution
In water, a substance that partially ionizes in solution is called a In water, a substance that partially ionizes in solution is called a semiconductor. weak electrolyte. nonconductor. strong electrolyte. nonelectrolyte.
weak electrolyte
NH3(g)+H2O(l)⇌ H2ONH4+(aq)+OH−(aq) strong electrolyte nonelectrolyte weak electrolyte
weak electrolyte You can tell because the arrows go both ways!! Also, doesn't completely disassociate.
Part complete What volume of 0.10 M NaOH can be prepared from 250. mL of 0.30 M NaOH?
0.75L Use: M1V1 = M2V2
Part complete What is the [OH-] in a solution that has a [H3O+] = 1 × 10-6 M? What is the [OH-] in a solution that has a [H3O+] = 1 × 10-6 M? 1 × 10-2 M 1 × 10-6 M 1 × 10-10 M 1 × 10-12 M 1 × 10-8 M
1 × 10-8 M
In which of the following are the pH values arranged from the most acidic to the most basic? In which of the following are the pH values arranged from the most acidic to the most basic? 2, 5, 7, 9, 10, 1.1 14, 10, 7, 4, 3, 1 7, 10, 14, 4, 3, 1 1, 3, 6, 8, 11, 14 14, 10, 7, 1, 3, 5
1, 3, 6, 8, 11, 14
How many grams of LiCl is present in 1.5 L of 2M solution? Question 7 options: 127.5 g 3 g 270 g 60 g
127.5g
What is the concentration, in m/v percent, of a solution prepared from 50. g NaCl and 2.5 L of water? 0.050% 20.% 5.0% 2.0% 0.020%
2.0 %
Given that the pH of a solution is 6.7, what is the [H3O+]? View Available Hint(s) Given that the pH of a solution is 6.7, what is the [H3O+]? 1.9953 × 10-7 M 2.0 × 10-7 M 8.0 × 10-1 M 5.0 × 106 M
2.0 × 10-7 M
What is the molarity of a solution which contains 58.5 g of sodium chloride dissolved in 0.500 L of solution? 1.00 M 1.50 M 4.00 M 2.00 M 0.500 M
2.00 M
The [OH-] of a solution with pH = 8.34 is 2.2 × 10-9 M. 2.2 × 10-6 M. 4.6 × 10-9 M. 3 × 10-6 M. 5 × 10-9 M.
2.2 × 10-6 M
What is be the concentration of solution if 20 ml water was added to 25 ml of 4 M KNO3 solution 22 M 4 M 2.2 M 5 M
2.2M
What is the pH of a solution with [H3O+] = 3.0 × 10-3 M? What is the pH of a solution with [H3O+] = 3.0 × 10-3 M? 3.0 × 10-3 -2.52 9.0 3.0 2.52
2.52
Part complete What volume of 2.5% (m/v) KOH can be prepared from 125 mL of a 5.0% KOH solution?
250 ml Use: M1V1 = M2V2
How many ml of 10% m / v glucose solution are need to get 25 g of glucose? Question 5 options: 100 ml 250 ml 500 ml 1000 ml
250ml???? 10g/100ml = 25g/?ml
How many mL of 0.246 M Pb(NO3)2 are needed to react with 36.0 mL of 0.322 M KCl? 2KCl(aq) + Pb(NO3)2(aq) → 2KNO3(aq) + PbCl2(s) 23.6 mL 47.1 mL 18.0 mL 36.0 mL 72.0 mL
????? See Class notes
How would you prepare a 10 ml of a 0.25 M HCl solution if 1 M was available? How much distilled water is needed, how much of the 1 M HCl is needed?
?????? 20mL Use C1V1 = C2V2 C1 = 1M V1 = ? C2 = .25M V2 = 10mL V1 = 2.5mL & need 7.5ml DI water.
how many ml of C2H5OH are needed to prepare a 1 Liter of 5% v/v solution., and how many ml of water will be needed. Question 10 options: 5 ml C2H5OH and 9.5 ml water 50 ml C2H5OH and 950 ml water 50 ml C2H5OH and 1000 ml water 5 L C2H5OH and 9.5 L water
??????? 50 ml & 950 ml water
A solution which has [OH-] = 3.4 × 10-12 M is A solution which has [OH-] = 3.4 × 10-12 M is acidic. basic. neutral.
acidic
The solubility of a solid ____________________ with decreasing temperature while the solubility of a gas _____________________ with decreasing temperature. (increases or decreases)
decreases; increases
According to Henry's law, the solubility of a gas in a liquid - decreases as the gas pressure above the liquid increases. - remains the same as the temperature increases. - depends on the liquid density. - depends on the liquid polarity. - increases as the gas pressure above the liquid increases.
increases as the gas pressure above the liquid increases.
Predict is the following ionic compounds is soluble in water? Ag2O
insoluble
Predict is the following ionic compounds is soluble in water? CaSO4
insoluble
Predict is the following ionic compounds is soluble in water? NiS
insoluble
1. NH4Cl, a strong electrolyte
ions only
1.0 mole of NaCl is added to 1.0 kg of water. The freezing point of the solution will be __________ the freezing point of pure water. higher than lower than the same as
lower than
Which of the following substances is a base when dissolved in water, as defined by Arrhenius? View Available Hint(s) Which of the following substances is a base when dissolved in water, as defined by Arrhenius? magnesium sulfate magnesium hydroxide magnesium chloride magnesium acetate
magnesium hydroxide
3. HCN, hydrocyanic acid, a weak electrolyte
molecules and a few ions
2. ethanol, C2H5OH, a nonelectrolyte
molecules only
Identify which of the following substances is an insoluble salt. -silver nitrate -silver chloride -sodium sulfate -ammonium chloride -ammonium nitrate
silver chloride
Predict is the following ionic compounds is soluble in water? Na2S
soluble
Predict is the following ionic compounds is soluble in water? NaI
soluble
The process that occurs in this system is above?
osmosis
In a sulfuric acid solution, where the [H3O+] is 0.01 M, what is the pH? pH = 12.0 pH = 5.0 pH = 3.0 pH = 11.0 pH = 2.0
pH = 2.0
How would you prepare a 10 ml of a 0.25 M HCl solution if 1 M was available? How much distilled water is needed, how much of the 1 M HCl is needed?
Use C1V1 = C2V2 C1 = 1 M C2 = 0.25 M V1 = ? V2 = 10mL Thus, 2.5 mL of 1 M HCl Solution will be required to prepare a 10mL solution of 0.25M HCl. Since the final solution volume is 10mL, the other 7.5mL (after adding 2.5 mL 1M HCl) will be made up of distilled water. So... to prepare 10mL, 0.25M HCl solution, add 7.5mL distilled water to 2.5ml, 1M HCl.
Consider the concentrations for both H3O+(aq) and OH−(aq). Which set of concentrations would result in a neutral solution? View Available Hint(s) Consider the concentrations for both H3O+(aq) and OH−(aq). Which set of concentrations would result in a neutral solution? [H3O+] = 1.6 × 10−12 M[OH−] = 6.2 × 10−3 M [H3O+] = 1.0 × 10−8 M[OH−] = 1.0 × 10−6 M [H3O+] = 3.6 × 10−4 M [OH−] = 2.8 × 10−11 M [H3O+] = 1.0 × 10−7 M[OH−] = 1.0 × 10−7 M
[H3O+] = 1.0 × 10−7 M[OH−] = 1.0 × 10−7 M
Which one of the following is characteristic of a base? Which one of the following is characteristic of a base? turns blue litmus red has a sour taste produces H3O+ in water has a slippery, soapy feel is insoluble in water
has a slippery, soapy feel
0.50 mole of KCl is added to 2.0 kg of water. The boiling point of the solution will be ________ the boiling point of pure water. higher than lower than the same as
higher than
Are the following solutions isotonic, hypotonic, or hypertonic compared with a red blood cell? 15% (m/v) glucose hypertonic isotonic hypotonic
hypertonic
Are the following solutions isotonic, hypotonic, or hypertonic compared with a red blood cell? 1 % (m/v) glucose hypotonic isotonic hypertonic
hypotonic
Are the following solutions isotonic, hypotonic, or hypertonic compared with a red blood cell? distilled H2O? hypertonic isotonic hypotonic
hypotonic
C6H12O6(s)⟶ H2OC6H12O6(aq) weak electrolyte nonelectrolyte strong electrolyte
non electrolyte
a mixture that settles out upon standing characteristic of a suspension characteristic of a colloid characteristic of a solution
suspension
Electrolyte
- substance that contains free ions - conducts electricity - can be strong, weak, Non
Part complete For Kw, the product of [H3O+] and [OH-] is For Kw, the product of [H3O+] and [OH-] is 1.0 × 10-7. 1.0 × 1014. 1.0 × 10-1. 1.0 × 10-14. 1.0.
1.0 × 10-14.
Rubbing alcohol is 70.% isopropyl alcohol by volume. How many mL of isopropyl alcohol are in a 1 pint (473 mL) container? 330 mL 0.15 mL 680 mL 70. mL 470 mL
330 mL
Which starch solution will decrease in volume as osmosis occurs? - 4% - 10% - Neither exerts osmotic pressure. - They exert equal osmotic pressures. - They exert opposite osmotic pressures.
4%
1) The O-H bond in water is polar because: A) it is an ionic bond. B) oxygen is much more electronegative than hydrogen. C) oxygen occupies more space than hydrogen. D) hydrogen is much more electronegative than oxygen. E) it is a hydrogen bond.
B) oxygen is much more electronegative than hydrogen. * it does not contain hydrogen bonds within the H20 molecule. Hydrogen bonds can only be BETWEEN molecules.
Part complete Which of the following is a nonelectrolyte? Which of the following is a nonelectrolyte? H2O NaCl NaOH C6H12O6 (glucose)
C6H12O6 (glucose)
Part complete The correct formula for sulfuric acid is The correct formula for sulfuric acid is H2SO3. SO42-. H2SO4. H2SO3-. H2SO4-.
H2SO4
When solutions of NaCl and AgNO3 are mixed,-- -no precipitate forms. -a precipitate of NaNO3 forms. -a precipitate of AgCl2 forms. precipitate of NaNO3 and AgCl form. -a precipitate of AgCl forms.
a precipitate of AgCl forms.
Which of the following is an example of a solution? Gatorade oil-based paint milk lemonade with pulp
Gatorade
The conjugate acid of HSO4- is HSO3-. HSO4. SO42-. H2SO4. H2SO4-.
H2SO4. When given Base and need conjugate acid - Add an H+ When given Acid & need conjugate base - subtract an H+ The basic thing is that conjugate pairs differ by a proton i.e H+ Lets take an example We have an acid, say H2SO4 Acid has a tendency to loose H+ So now H2SO4 looses a H+ ion and what forms as a reault of it is HSO4- Here HSO4^- is the conjugate base So all this can be summed up as Acid~~~> H^+ + conjugate base Similarly base +H^+ ~~~~> conjugate acid So in exam just remove 1H+ whenever conjugate base is asked andd add 1H+ when conjugate acid is asked.
Part complete Identify the conjugate acid-base pairs in the following reaction: HCl+NH3→NH4++Cl− Identify the conjugate acid-base pairs in the following reaction: HCl/NH4+ and NH3/Cl− HCl/NH3 and NH4+/Cl− HCl/Cl− and NH4+/NH3
HCl/Cl− and NH4+/NH3
Which of the following sets of chemicals is an acid-base conjugate pair? H2O(aq) & HClO2(aq) H3O+(aq) & ClO2 ¯(aq) HClO2(aq) & ClO2 ¯(aq) HClO2(aq) & ClO¯(aq)
HClO2(aq) & ClO2 ¯(aq)
What ions will be present in the solution when KOH was allowed to react with HCl? K+ , O-2, H+, Cl- K+, OH-, H+ , Cl- KCl, H2O K+ , Cl-
K+, Cl-
Part complete A solution is prepared by dissolving 2 g of KCl in 100 g of H2O. In this solution, H2O is the
Sovent
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, the solution will start boiling. the solution will freeze. the solution will be unsaturated. a saturated solution will form. all of the KI will dissolve.
a saturated solution will form.
Part complete Oil does not dissolve in water because
Oil is nonpolar
30.00 mL of water is added to 20.00 mL of 0.0500 M sodium carbonate. What is the molarity of sodium ions in the new solution? Na2CO3 (Sodium Carbonate)
The molarity of Na+ is approximately 0.0400M. (30.00 mL of water added to 20.00 mL of solution gives you approximately 50.00 mL of solution. Remember that volume is not additive. By applying the M1V1 = M2V2 equation, the answer gives you the molarity of sodium carbonate. You need to know the formula of sodium carbonate. It is Na2CO3 because it tells you that for each unit of Na2CO3 there are two Na+. Thus the concentration is doubled: After applying the M1V1 = M2V2 equation, you get M2 = 0.0200 M Na2CO3. Ans. is 0.0400 M Na+
Which of the following occurs in this system? - Water does not cross the membrane at all. - Starch moves out of the 10% starch solution into the 4% starch solution. - There is a net flow of water from the 4% starch solution into the 10% starch solution. - Water flows equally in both directions. - There is a net flow of water from the 10% starch solution into the 4% starch solution.
There is a net flow of water from the 4% starch solution into the 10% starch solution.
The mass percent concentration refers to -grams of solute in 1 kg of solvent. -grams of solute in 100 g of solvent. -grams of solvent in 100 g of solution. -grams of solute in 100 g of solution. -grams of solute in 1 kg of solution.
grams of solute in 100 g of solution.
The mass/volume percent concentration refers to-- -grams of solvent in 100 mL of solution. - grams of solute in 1 L of solvent. - grams of solute in 1 L of solution. - grams of solute in 100 mL of solution. - grams of solute in 100 mL of solvent.
grams of solute in 100 mL of solution.
In water, a substance that ionizes completely in solution is called a In water, a substance that ionizes completely in solution is called a semiconductor. nonconductor. strong electrolyte. weak electrolyte. nonelectrolyte.
strong electrolyte
K2SO4(s)⟶ H2O2K+(aq)+SO42−(aq)
strong electrolyte
