What volume of the stock solution (Part A) would contain the number of moles present in the diluted solution (Part B)
What volume of the stock solution (Part A) would contain the number of moles present in the diluted solution (Part B)? Express your answer with the appropriate units. .979 molarity of luminol solution and 8.00*10-2 moles of luminol
1.The concentration of the diluted solution determined in part b
and in part c must be equal. how do the values obtained compare?
explain
part b: preparation of a dilution solution
standard solution volume used: 10.00 mL
final volume of the solution: 25.00 mL
concentration of the standard solution:
0.800 mol/L
part c: experimental determination of the concentration of the
diluted solution
dough test tube with residue: 46.19g
dough test tube empty: 47.42g
volumen of solution used: 3.00mL or 0.003L...
1.Calculate the number of moles of solute present in am aqueous
solution of 86.3 g of 0.160 m KCl.
2. The density of toluene (C7H8) is 0.867g/mL, and the density
of thiophene (C4H4S) is 1.065 g/mL. A solution is made by
dissolving 9.38g of thiophene in 270 mL of toluene. Calculate the
(a) percentage and (b) Molality of thiophene.
3a) How many mL of a 1.21 M NaOH solution would contain 0.275
moles of NaOH? ___ mL NaOH solution
3b) How many mL of 12M HCl solution is needed to prepare 775mL
of 0.880M HCl by dilution? ___ mL is needed.
3c) Calculate the molarity of a solution made by dissolving
35.2g K2CO3 in enough water to form 275mL of solution. The solution
is ____ M.
3d) 10.5mL of 12M HCl solution is diluted to a volume of 122mL....
A) 7mL of a 0.1M CaCl2 solution was diluted to a final volume of
150mL. Please determine the concentration of Cl- in this
solution.
B) Explain why creating a
standard curve is better than simply using the Beer-Lambert law
directly. Assume that a value for molar absorptivity is readily
available.
queous KNO3 solution is made using 84.7 g of KNO3 diluted to a
total solution volume of 2.06 L . (Assume a density of 1.05 g/mL
for the solution For this solution, calculate percent by mass For
this solution, calculate mole fraction.
One deciliter of a .9% nickel (II) nitrate solution is diluted
to a volume of 500 mL. Calculate the final [NO3-] of the resultant
solution. Answer in M please.
Determine the volume, in miliiters, required to prepare each of the
following diluted solutions:
Part A: 252 mL of a 0.200 M HNO3 solution from a 4.30 M HNO3
solution
Part B: 719 mL of a 0.100 M MgCl2 solution using a 5.50 M
MgCl2 solution
Part C: 0.150 L of a 0.150 M KCl solution using an 8.40 M KCl
solution