Calculate the final concentration of the solution in each of the following. Part

Question

Calculate the final concentration of the solution in each of the following.
Part A: Water is added to 0.180 L of a 4.60 M HCl solution to give a volume of 1.00 L.
Part B: A 20.0 mL sample of a 4.00 M KCl solution isa diluted with water to 0.300 L.
Part C: Water is added to 0.400 L of a 10.7 M KBr solution to give a volume of 0.900 L. Part A Problem 12.43 Water is added to 0.180 L of a 460 M HCI solution to give a vokime of 1.00L Express your answer with the appropriate units Calculate the final concentration of the solution in each of the following uA Value Units Submit My Answers Give Up Part B A 20 0 ml sample of a 4.00 M KCl solution isa dluted with water to 0.300 L Express your answer with the appropriate units Value Units Submit My Answers Give Up

Explanation / Answer

In order to calculate moles you need to remember that:

moles = Volume(L) x Molarity(mol/L)

A) moles HCl = (0.180L)(4.60M) = 0.828moles

Now these moles are in 1.00L, then M = 0.828moles/1.00L = 0.828M

b) Here, you need convert 20.0ml to L : 20.0ml(1L)/(1000ml)= 0.0200L

moles KCl= (0.0200L)(4.00M) = 0.0800moles. But they were diluted to 0.300L :

M = 0.0800moles/0.300L = 0.267M.

C) moles KBr= (0.400L)(10.7M)= 4.28moles But they are diluted in 0.900L:

M=(4.28moles)/(0.900L)= 4.76M.

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