# Solutions Worksheet #1 Molarity Solute formula Mass of Solute by murplelake75

VIEWS: 8,356 PAGES: 3

• pg 1
```									Name _________________________________________ Date____________ Period _______

Solutions Worksheet #1: Molarity
1) Complete the table:
Solute      Molar Mass of         Mass of          Moles of        Molarity of     Volume of
formula solute (g/mole)           Solute (g)      solute (mole)     solution (M)    solution (L)
a       NaCl            58.5              58.5              1               1.0                1.0
b       NaOH                              117.0                                                4.0
c       MgCl2           95.3              190.3             2               1.0                2.0
d       NaCl                              292.5                             0 .5
e        KBr            119               238.0             2               2.0                1.0
f       NaCl                                                                1.5                1.0
g       NaCl            58.5              14.63             0.25            1.0                0.25
h       FeCl3                                                               0.1                0.50
i        HCl            36.5              438.0             12              6.0                2.0
j        NH3                              39.1                              3.0

2) Calculate the number of moles and the number of grams of solute in each solution:
Moles of solute      Molar Mass of solute       Mass of solute
(mol)                 (g/mol)                   (g)
a    1.0 liter of .5 M NaCl               .5                     58.5                   29.3
b    500.0 mL of 2.0 M KNO3
c    250.0 mL of .10 M CaCl2              .025                     111                     2.78
d    2.0 liters of .30 M Na2SO4

3) Compute the mass of solute needed to make 500.0 mL of solution at the indicated molarity.
a: 0.5M sulfuric acid 24.5g           e: 0.1M iron III chloride   8.125g
b: 0.01M HNO3                         f: 3M NH3
c: 6.0M HCl 109.5g                     g: 5.0M KOH    140.0g
d: 0.50M sodium hydroxide

4) How many moles of H2SO4 are in 1.00 liter of a 1.55M H2SO4 solution? How many grams?

5) How many grams of sodium sulfate are contained in 1.50L of .25M solution? 53.25g Na2SO4

6) How many grams of ammonium sulfate are required to prepare 3.50L of a 1.55M solution?

7) How many moles of sodium chromate are contained in 1.75 L of a 2.00M solution?
3.5 mol NaCr2O7
8) A sample of glucose (C6 H12O6) is dissolved in water. How many moles of glucose are
dissolved in 200.0 ml of solution if its concentration is .150M?

9) A mass of 98g of sulfuric acid are dissolved in water to prepare a .50M solution. What is
the volume of the solution, in liters? 2L

10) What is the molarity of a solution of HNO3 that contains 12.6g of solute in 500ml of
solution?
Name ______________________________________ Date____________ Period _______

Solutions Worksheet #2: Molarity and Dilution Problems

1) Describe how you would prepare 5.00 liters of a 6.00M solution of potassium hydroxide.
g= M . L. g/moles = (6.00M) (5.00L) (56.0g/mol) = 1.68 g   mass out 1.68g KOH, put in flask & fill to 5L with
dH2O
2) How would you prepare 100.0ml of .4M MgSO4 from a stock solution of 2.0 MgSO4?

3) If 1.00L of water is added to 3.00 L of a 6.00M solution of HCl, what is the new molarity
of the acid solution?
M1V1 = M2V2   (6.00M) (3.00L) = M2 (4.00L)     M2=4.50M

4) What is the concentration when 50.0ml of 1.0M Na2SO4 is diluted to 500mL?

5) How would you prepare 4.0L of .5M sodium carbonate from a 10.0M solution?
(.5 M)(4.0L) = (10.0M) V2     .2 L of 10.0 M solution and fill to 4.0 L with dH2O

6) You need 267 mL of .25M NaCl, but the only supply of NaCl you have is 1.75M NaCl. How do
you prepare the required solution?

7) Describe how you would prepare 1.50L of a .25M solution of sodium sulfate.
g= M . L. g/moles = (.25 M) (1.50 L) (142 g/mol) = 53.g
mass out 53g of Na2SO4 & put in flask, fill to 1.5 L with dH2O

8) Calculate the molarity of a solution containing 10.0 grams of sulfuric acid in 500 ml of
solution.

9) Hydrogen peroxide solution for hair bleaching is usually prepared by mixing 5.0 go of
hydrogen peroxide, H2O2, per 100.0 ml of solution. What is the molarity of this solution?
Mol = 5.0g / 34 g/mol = .15 mols H2O2      O.15 mol / .10L = 1.5 mol/L

10) A chemist wants to dilute 50.0 ml of 3.50 M Sulfuric acid to 2.00 M Sulfuric acid. To
what volume must it be diluted?
Name ________________________________________________ Date _____________ Period ____________
Solutions Worksheet #3: Electrolytes

Directions: Use the words provided to fill in the blank spaces below.
water        positive                electrolyte          negative        move
sugar        neutral                 nonelectrolyte       ions            electric current
voltage      volts                   electric charge      amps            sodium chloride

1)   Substances that dissolve in water are classified according to whether they produce molecules or
_ions______in solution.

2) When an ionic compound dissolves, the ____________ and ____________ ions separate from each
other and are surrounded by ________________molecules.

3) These solute ions are free to_____move__, making it possible for an _____electric current________
to pass through the solution.

4) Current is the flow of ______________________ which is measured in ______________.

5) _voltage_____ is the push or pull of electrons in a wire measured in ____amps___.

6) A substance that dissolves in water to give a solution that conducts electric current is called an
__________________.

7) __NaCl______is an example of an electrolyte.

8) A solutions containing _________ solute molecules does not conduct electric current because it does
not contain mobile charged particles.

9) A substance that dissolves in water to give a solution that does not conduct an electric current is
called a non-electrolyte_________.

10) _________________ is an example of a nonelectrolyte

Directions: Complete the following table
Solution        Cation          Cation        Anion          Anion           Total Ion
concentration      Formed       Concentration   formed      Concentration     Concentration
11)      1.0 M NaCl               Na+             1.0 M          Cl-           1.0 M             2.0 M

12)      1.0 M Al(OH)3
13)      2.0 M NaOH               Na+             2.0 M         OH-            2.0 M             4.0 M

14)      2.0 M MgBr2
15)      0.10 M KCl                K+             .10 M          Cl-           .10 M             .2 O M

16)      0.10 M K2SO4
17)      0.10 M K3PO4              K+             0.3M          PO4             .1M               .4M

18)      0.50 M LiCl
19)      0.50 M CaCl2             Ca2+            .50 M          Cl-           1.0M              1.5M

20)      0.50 M C6H6O6

```
To top