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- If you add more solvent to a solution, then the concentration of the soution decreases
M1V1 = M2V2
M = molarity (mol/L)
V = volume (L)
ex) If you dilute a 1.6M LiCl solution from 175 mL to 1.00L, what will be the new concentration?
M1V1 = M2V2
M1 - 1.6m
V1 - .175L
M2 - ?
V2 - 1.00L
(1.6M)(.175L) = M2 (1.00L)
M2 = .28M
Ex) How many mL of 5.0M CuSO4 do you need to make a 160mL solution 0.3M in concentration?
M1V1 = M2V2
(5.0M)V1/5M = (0.3M)(.160L)/5M
V1 = .0096L = 9.6mL
Ex) How much H20 should be added to a .5M solution with a volume of 150mL to make it 1/10 in concentration?
(.5M)(V1)/.5M = (.10M)(.150L)/.5M
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Precipitation Chemistry
NaCl(aq) + AgNO3(aq) --> AgCl (s) NaNO3(aq)
- We want to be able to predict the mass of the precipitate prior to the mixing of solutions.
Ex) A 0.5M NaCl solution (100mL) is reacted with 50mL of a 0.1M AgNO3 solution. What mass of AgCl3 should form?
NaCl + AgNO3 __> AgCl + NaNo3
NaCl = 0.5M, 100mL..... 0.5M= X/.100L.... X = .05mol NaCl
AgNO3 = 0.1m, 50mL... 0.1M = X/.05L ... X = .005 mol AgNo3 LR
Long equation..... = .717g AgCl
Ex2) CuSO4(aq) + 2NaOH(aq)--> Cu(OH)2 (S) + NA2SO4(aq)
CuSO4 (aq)= .5m, 20mL.... .5M= x/.020L.... X= .
2NaOH (aq)= .3m, 30mL... .3M= x/.030L.... X= .
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