When preparing . 0.500 M solution of Manganese Sulfate Monohyrate. you accidentl
ID: 913833 • Letter: W
Question
When preparing . 0.500 M solution of Manganese Sulfate Monohyrate. you accidently tetri hydrate form Explain what effect this has on your final concentration revive .o sou, uree. concentration? You have a 6.00 M stock solution of NaCI. Your goal is to make a 250.00 ml. solution of 0.750 M NaCI. What specifie (be quantitative) steps will you lake to make this desired solution. You add 400 ml. of a 30% hydrogen peroxide solution to 600 ml. of water What is sour final concentration of hydrogen peroxide (as a percentage).Explanation / Answer
5) Molarity = 0.500 M
In order to make 0.500 M solution of Manganese Sulphate monohydrate we need 0.500 moles of Manganese Sulphate monohydrate in 1 L of solution it means as follows
0.500 = w/M = w/169.02
w = 84.51 g of Manganese Sulphate monohydrate in 1000 mL of solution.
But if instead of Manganese Sulphate monohydrate we used tetrahydrate form then the concentration will automatically vary because molecular weight vary and then the final concentration will become as follows if we add the same amount of weight as above = 84.51 g
M = 84.51/223.06 = 0.378 Molar so this concludes the final concentration will decrease.
6) We are provided with 6 M stock NaCl solution. We want to make 250 mL solution of 0.750 M of NaCl. This means we just need to calculate the amount (volume) of NaCl which we need to make the 250 mL solution of 0.750 M of NaCl as follows.
M1 x V1 = M2 x V2
6 x V1 = 0.750 x 250
V1 = 31.25 mL OF 6 M NaCl we will and dilute it to 250 mL to make solution.
7) 30% H2O2 means 30 grams of H2O2 in 100 mL of solution
120 grams of H2O2 in 400 mL of solution and if we add 600 mL water more then that means 120 grams of H2O2 in 1000 mL of solution so final concentration of H2O2 will decrease and becomes 0.12% H2O2.
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