Chemistry related question?

How many grams are in 750 mL of a 17.5% BaBr2 solution?

Also,

You prepare a solution by placing 42.5 g of CaCl2 in 500 mL of solution. Then, dilute that solution to 0.25M. How much of the 0.25M solution could be made?

Answer:
You need to know the density of the BaBr2 solution to get the answer.
750 mL x density (g/ml) x .175 = grams of BaBr2

42.5 gm of CaCl2 is 42.5 / 110.99 = 0.3829 moles
(110.99 is the MW of CaCl2)

Liters x Molarity = Moles
Liters x 0.250 = 0.3829
Liters = 1.532 = 1,532 mL
Well if you have a 17.5% solution the you have 17.5g/100mL or 175g/1000mL So if you have 750mL of solution then you have:

175g*0.75=131.75grams



42.5g*(1moleCaCl2/110.984g)=0.

Then you use the equation Mconc*Vconc=Mdiluted*Vdiluted

(0.766M*0.5L)=(0.25M*x) Solve for x

x=1.532Liters so approximately 1.5Liters

The answers post by the user, for information only, FunQA.com does not guarantee the right.



More Questions and Answers:
  • Is restoring rancid butter safe?
  • What are the chemical changes in burning of a candle?
  • Last one before I sleep! Solubility Question! Quick!?
  • I would l;ike to know the importance and meaning of Dew Point temperature in Crude Unit coloumn operation?
  • Does tobacco contain chemical form of Alcohol?
  • The windscreen of a car broke during a hot afternoon?
  • Electrochemistry- using the Nernst Equation?
  • What is the definition of bouyancy error?
  • In solar panels what does doping the silicon crystals mean (with boron)?