1.(a) A 20.0 L container at 303 K holds a mixture of two gases with a total pressure of 5.00
here are 2.00 mol of Gas A in the mixture, how many moles of Gas B are present? (R = 0.0821 L • atm/(K • mol))
(b) The gas in a 250. mL piston experiences a change in pressure from 1.00 atm to 2.80 atm. What is the new volume (in mL) assuming the moles of gas and temperature are held constant?
(c) Small quantities of Oxygen can be produced by the decomposition of mercury(II) oxide as shown below. Typically, the oxygen gas is bubbled through water for collection and becomes saturated with water vapor. Atomic weight of HgO = 216.6 amu, Atomic weight of Oxygen = 32.00 amu)
2 HgO(s) → 2 Hg(ℓ) + O₂(g)
(i) Assuming that 3.05 grams of HgO was used in this reaction, determine the number of moles of oxygen gas formed.(According to the above chemical equation)
(ii) Assuming 310. 0 mL of Oxygen gas was collected at at 29°C, calculate the pressure of the Oxygen gas that was collected. (R = 0.0821 L • atm/(K • mol)
(iii) If the vapor pressure of water at this temperature equals to 0.042 atm, calculate the pressure reading of this experiment.
5.5 (5 points) There is H3PO4 available in stock solution that has an assay of 77% and a density
cific gravity) of 1.24. What is the molarity of this solution?
Using this solution how would 1 L of 2N solution be made.
6 (5 points) H3BO3 is needed to neutralize 20 ML of a 2N solution of NaOH. How much of the acid should I put in 40 ML of the water to exactly neutralize this solution?
7 (6 points) Describe how to make the solutions below :
20% w/v Salt in water.
20% v/v alcohol in water
20% w/w NaCl in water.
8 (three points) I have 0.6 g/dl solution of NaOH. What is M? Whan is N?
9 (six points) There are 3000mL of 3M NaOH. How much of the following do I need to neutralize? (watch your M’s and N’s
a) 3M H3PO4
b) 2M H2SO4
c) 1M HCL
10 (20 points) The following solutions of NaOH are mixed together 20ML of 3N, 40mL of 2N, 60mL of 1N, 80 mL of 4N, and 100mL of 5N.
a) What is the volume and normality of the final solution?
b) How much 4M sulfuric acid would I need to neutralize?
c) How much stock solution of sulfuric acid with an assay of 77% and a specific gravity of 1.14 would I need?
d) How many grams of HCl would I have to put in a 300mL solution of HCl in water to neutralize?
11 (3 points) How much 5N solution can I make with 98 grams of H3PO4 ?
12 (5 points) How much 5N solution of H3AsO4 can I make with 57 mL of stock solution that is 84% assay and 1.14 specific gravity?
13 (5 points) If we have a 4N solution of HCl that has 0.03645g of HCl in the solution, how many microliters of solution do we have?
14 (10 points) If we have 66mL of a solution of concentrated NaOH that has an assay of 88% and a specific gravity of 1.24, how much 3N H3AsO4 can be neutralized?
15 (ten points) If I have 17 mL of a 20% w/v solution of NaOH and I want to neutralize with H2SO4 that is available in a 4% w/v solution, how much of this solution will be required.
16 (ten points)
a) I have an 12mL of Ba(Cl)2 that is 78% assay that contains 8 grams of Ba(Cl)2. What is the specific gravity?
b) How many Moles of Ba(Cl)2 are there?
c) If I have 80 grams of NaOH in a liter of solution that is of an unknown specific gravity, can I calculate molarity and what is it?
d) What is the difference between molarity and normality?
e) I have 77 ml of 77% salt in water. How much 11% can I make?