Which of the following gives the molarity of a 17.0 % by mass
solution of sodium...
Which of the following gives the molarity of a 17.0 % by mass
solution of sodium acetate, CH3COONa (molar mass = 82.0 g/mol) in
water? The density of the solution is 1.09 g/mL.
1. What is the molarity of a 12.6% solution of sodium
carbonate with a density of 1.31 g/mL?
2. What is the mass percent of potassium iodide in a
2.89 M solution of KI with a density of 1.27 g/mL?
3. In an experiment similar to your 15.72 mL of a 0.1294
M Ba(OH)2 solution is titrated with 20.00 mL of a HNO3 solution.
What is the molarityof the HNO3?
What is the molarity of a solution made by adding 18.00 mL of
5.00 M sodium acetate to 55.00 mL of water? I got 1.64 as the
molarity but when i enter that answer it says it is wrong, so i
must be doing something wrong. Can you help?
Complete the following table:
Mass
Mol
Volume
Solute
Solute
Solute
Solution
Molarity
KNO3
23.5g
_____
127.0mL
_____
NaHCO3
_____
_____
260.0mL
0.150M
C12H22O11
57.38g
_____
_____
0.120M
Part A
Complete the row for KNO3.
Enter your answers numerically separated by a comma.
Part B
Complete the row for NaHCO3.
Enter your answers numerically separated by a comma.
Part C
Complete the row for C12H22O11.
Enter your answers numerically separated by a comma.
What is the molarity of ethanol (C2H5OH) in a solution of
ethanol in water in which the mole fraction of C2H5OH is 0.144? The
density of the solution is 0.9566 g/mL.
How do you determine the mass needed to make a certain molarity
and certain pH solution? For example, if I need to make 300 mL of
0.05 M Tris Base and 0.05 M NaCL (pH 8.2) from 2M of both, how do I
do the math for that and get the grams needed of each?
Also how do you use the Henderson-Haseelbach equation to
determine how much .1 M KH2PO4 to add to 100 mL of of K2HPO4 to
give...
An unknown mass of sodium hydroxide is dissolved in 500 g of
water. This solution is neutralized by adding successively 18 g of
CH3COOH, 25.2 g HNO3, and 29.4 g of H2SO4. Determine
a) the mass of NaOH
b) the mass of H2O in the neutral solution.
Which of the following gives a buffer solution when equal
volumes of the two solutions are mixed?
(a) 0.10 MHF and 0.10 MNaOH
(b) 0.20 MHF and 0.10 MNaOH
(c) 0.10 MHCl and 0.20 MNaF
(d) 0.10 MHF and 0.10 MNaF