Help with Concentration of unknown solute?
1. Hydrochloric acid is purchased as 11.7M How do you create a 500mL sample of 0.1M hydrochloric acid?
2) How do you create 250ml of a 0.1M of silver nitrate?
3) If you dissolve 5.67g of ferric nitratre into 325mL of water, what is the concentration of the final solution?
Any help would be apprieciated :)
Answer:
1) you figure out how many moles of HCl are there in 500ml of .1 M solution, then use that number to figure out how many ml of the original 11.7 M solution you need
hint M means moles per 1000ml
1000ml= 1 liter
2) same as above, figure out how many moles of silver nitrate in 250ml of .1M solution
3) Figure out how many moles of ferric nitrate you have and divide that by the volume giving you moles/liter which is M which is concentration
hope this helps, good luck
1) mL x M = mL x M
mL x 11.7 = 500 x 0.1
mL = 500 x 0.1 / 11.7
mL = 4.27
dissolve 4.27 mL of 11.7 M HCl in enough water to make 500 mL of solution.
2) 0.1 M Silver Nitrate means that 1 liter (1000 mL) of solution contains 0.1 mole of AgNO3. The molar mass of AgNO3 is 107.88 + 14.008 + 3 x 16 = 169.888
1000 mL of 0.1 M AgNO3 would contain 16.9888 g of AgNO3. 250 mL would contain (250/1000) x 16.9888 or 4.2472 g. Dissolve 4.2472 g of AgNO3 in enough water to make 250 mL of solution.
3) Ferric Nitrate is Fe(NO3)3 and has a molar mass of 241.87 g per mole. 5.67 g would be 5.67/241.87 or 0.02344 moles of Fe(NO3)3. 02344 moles per 0.325 mL = 0.0721 moles per 10-00 mL so you solution was 0.0721 Molar.
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