1.3d calculate the amount of substance in a solution of known concentration

You should also be able to use the equation moles = volume x concentration and perform basic titration calculations.
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CALCULATIONS BASED ON CONCENTRATIONS IN SOLUTION
(These were summer homework so I only did odd questions)

Calculate the number of moles in each given volume of solution.
1. 25cm3 of 1.0mol dm-3 HCl
cm3 into dm3 = 25/1000 = 0.025
moles = volume x concentration = 0.025 x 1.0 = 0.025 moles
3. 250cm3 of 0.25mol dm-3 HCl
cm3 into dm3 = 250/1000 = 0.25
moles = volume x concentration = 0.25 x 0.25 = 0.0625 moles
5. 25cm3 of 1.0mol dm-3 NaOH
cm3 into dm3 = 25/1000 = 0.025
moles = volume x concentration = 0.025 x 1.0 = 0.025 moles
7. 50cm3 of 0.25mol dm-3 HNO3cm3 into dm3 = 50/1000 = 0.050
moles = volume x concentration = 0.050 x 0.25 = 0.0125 moles
9. 25cm3 of 0.05mol dm-3 KMnO4
cm3 into dm3 = 25/1000 = 0.025
moles = volume x concentration = 0.025 x 0.05 = 0.00125 moles

Calculate the mass of material in the given volume of solution.
11. 25cm3 of 1mol dm-3 HCl
cm3 into dm3 = 25/1000 = 0.025
moles = volume x concentration = 0.025 x 1 = 0.025 moles
mass = moles x RFM = 0.025 x (1+35.5) = 0.9125g 
13. 100cm3 of 0.25mol dm-3 NH4NO3
cm3 into dm3 = 100/1000 = 0.1
moles = volume x concentration = 0.1 x 0.25 = 0.025 moles
mass = moles x RFM = 0.025 x (4+48+28) = 2g
15. 25cm3 of 1mol dm-3 BaCl2
cm3 into dm3 = 25/1000 = 0.025
moles = volume x concentration = 0.025 x 1 = 0.025 moles
mass = moles x RFM = 0.025 x (137.3+71) = 5.21g
17. 20cm3 of 0.1mol dm-3 NaOH
cm3 into dm3 = 25/1000 = 0.020
moles = volume x concentration = 0.020 x 0.1 = 0.002 moles
mass = moles x RFM = 0.002 x (23+16+1) = 0.08g
19. 25cm3 of 0.02mol dm-3 KMnO4
cm3 into dm3 = 25/1000 = 0.025
moles = volume x concentration = 0.025 x 0.02 = 0.0005 moles
mass = moles x RFM = 0.0005 x (39.1+55+64) = 0.0791g 

Calculate the concentration in mol dm-3 of the following.
21. 3.65g of HCl in 1000cm3 of solution
cm3 into dm3 = 1000/1000 = 1
moles = mass/RFM = 3.65/(1+35.5) = 0.1 moles
concentration = moles/volume = 0.1/1 = 0.1mol dm-3
23. 6.624g of Pb(NO3)2 in 250cm3 of solution
cm3 into dm3 = 250/1000 = 0.25
moles = mass/RFM = 6.624/(207.2+28+96) = 0.02
concentration = moles/volume = 0.02/0.25 = 0.08mol dm-3 (I'm not sure why this is wrong)
25. 1.962g of H2SO4 in 250cm3 of solution
cm3 into dm3 = 250/1000 = 0.25
moles = mass/RFM = 1.962/(2+32.1+64) = 0.02 moles
concentration = moles/volume = 0.02/0.25 = 0.08mol dm-3 (I'm not sure why this is wrong either, even though they're identical)
27. 25g of Na2SO3.5H2O in 250cm3 of solution
cm3 into dm3 = 250/1000 = 0.25
moles = mass/RFM = 25/(46+32.1+10+128) = 0.116 moles
concentration = moles/volume = 0.116/0.25 = 0.464mol dm-3 (This one is wrong too, for some reason)
29. 4.80g of (COOH)2.2H2O in 250cm3 of solution
cm3 into dm3 = 250/1000 = 0.25
moles = mass/RFM = 4.80/(6+64+12) = 0.059 moles
concentration = moles/volume = 0.059/0.25 = 0.236mol dm-3 (also wrong, if anyone has any idea why, please comment)
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SIMPLE VOLUMETRIC CALCULATIONS

Calculate the molarity (the number of moles) of the first named solution.
1. 25cm3 of sodium hydroxide reacts with 21cm3 of 0.2 mol dm-3 HCl
NaOH + HCl --> NaCl + H2O
cm3 into dm3 = 21/1000 = 0.021
moles = concentration x volume = 0.021 x 0.2 = 0.0042 moles
- ratio
NaOH:HCl, 1:1, 0.0042
cm3 into dm3 = 25/1000 = 0.025
concentration = moles/volume = 0.0042/0.025 = 0.168 mol dm-3 
3. 20cm3 of hydrochloric acid reacts with 23.6cm3 of 0.1 mol dm-3 NaOH
HCl + NaOH --> NaCl + H2O
cm3 into dm3 = 23.6/1000 = 0.0236
moles = concentration x volume = 0.0236 x 0.1 = 0.00236 moles
- ratio
HCl : NaOH, 1:1, 0.00236 
cm3 into dm3 = 20/1000 = 0.020
concentration = moles/volume = 0.00236/0.020 = 0.118 mol dm-3 
5. 25cm3 of nitric acid reacts with 15cm3 of a solution of 0.2 mol dm-3  NH4OH
HNO3 + NH4OH --> NH4NO3 + H2O
cm3 into dm3 = 15/1000 = 0.015
moles = concentration x volume = 0.015 x 0.2 = 0.003 moles
- ratio
HNO3 : NH4OH, 1:1, 0.003 
cm3 into dm3 = 25/1000 = 0.025
concentration = moles/volume = 0.003/0.025 = 0.12 mol dm-3 
7. 25cm3 of a solution of NaCl reacts with 10cm3 of a 0.02 mol dm-3 silver nitrate
NaCl + AgNO3 --> NaNO3 + AgCl
cm3 into dm3 = 10/1000 = 0.010
moles = concentration x volume = 0.010 x 0.02 = 0.0002 moles
- ratio
NaCl : AgNO3, 1:1, 0.0002 
cm3 into dm3 = 25/1000 = 0.025
concentration = moles/volume = 0.0002/0.025 = 0.008 mol dm-3 
9. 25cm3 of HxA reacts with 25cm3 of 0.2 mol dm-3 NaOH to give Na2A
HxA + NaOH --> Na2A + H2O
cm3 into dm3 = 25/1000 = 0.025
moles = concentration x volume = 0.025 x 0.2 = 0.005 moles
- ratio
HxA : NaOH, 1:1, 0.005 
cm3 into dm3 = 25/1000 = 0.025
concentration = moles/volume = 0.005/0.025 = 0.02 mol dm-3 (this is probably due to me not working out the x)