H^+ = acid
OH^- = alkaline
Acids have a pH of below 7. The lower the number, the strongest the acid.
Once you have identified the limiting reactant, you calculate how much of the other reactant it must have reacted with and subtract from the original amount.
Answer:
0.8749 grams of hydrogen gas was formed from the reaction.
Explanation:
P = Pressure of hydrogen gad= 744 Torr = 0.98 atm
(1 atm = 760 Torr)
V = Volume of hydrogen gas= 11 L
n = number of moles of hydrogen gas= ?
R = Gas constant = 0.0821 L.atm/mol.K
T = Temperature of vapor = 27.0 °C = 300.15 K
Putting values in above equation, we get:
Using an ideal gas equation:
n = 0.4374 moles
Mass of 0.4374 moles of hydrogen gas:
0.4374 mol × 2 g/mol = 0.8749 g
0.8749 grams of hydrogen gas was formed from the reaction.
For all three questions, we will use the fact that
- molarity = (moles of solute)/(liters of solution)
1) For 175 mL of solution at 0.203 M, this means that:
- 0.203 = (moles of solute)/0.175
- moles of solute = 0.035523 mol
Considering the hydrochloric acid solution, if we have 0.035523 mol, then:
- 6.00 = 0.035523/(liters of solution)
- liters of solution = 0.035523/6.00 = 0.0059205 = <u>5.92 mL (to 3 sf)</u>
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2) If there is 20.3 mL = 0.0203 L, then:
- 8.20 = (moles of solute)/0.0203
- moles of solute = 0.16646 mol
This means that the molarity of the diluted solution is:
- 0.16646/(0.200) = <u>0.832 M (to 3 sf)</u>
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3) If we need 1.50 L of 0.700 M solution, then:
- 0.700 = (moles of solute)/1.50
- moles of solute = 1.05 mol
Considering the 9.36 M acid solution, from which we need 1.05 mol of perchloric acid from,
- 9.36 = 1.05/(liters of solution)
- liters of solution = 1.05/9.36, which is 0.11217948717949 L, or <u>112 mL (to 3 sf)</u>
