Question

to what volume should you dilute 50.0 mL of 5.00 M NaOH solution so that 25.0 mL of this diluted solution requires 28.5 mL of 1.50 M HCl solution to titrate?

Answer #1

To what volume should you dilute 130 mL of an 7.90 M CuCl2
solution so that 51.0 mL of the diluted solution contains 4.65 g
CuCl2? answer in mL

To what volume should you dilute 319 mL of a 6.70 M calcium
nitrate so that 44.5 mL of the diluted solution contains 1.972 g
calcium nitrate?

A 50.0-mL sample of a 1.50 M NaOH solution is titrated with a
2.90 M HCl solution. What will be the final volume of solution when
the NaOH has been completely neutralized by the HCl?

What volume of 0.100 M HCl is required to titrate 25.0 mL of
0.050 M NaOH?

To what volume should you dilute 20 mL of a 11 M stock HCl
solution to obtain a 0.580 M HCl solution?

1. If I have 100 mL of a 0.15 M NaOH solution and I dilute the
solution to a final volume of 250 mL, what will the molarity of the
diluted solution be?
2. If I add 25 mL of water to 125 mL of a 0.15 M NaOH solution,
what will the molarity of the diluted solution be?
3. I have 345 mL of a 1.5 M NaCl solution. If I boil the water
until the volume of the...

1)
A 21.30 mL volume of 0.0975
M NaOH was used to titrate 25.0
mL of a weak monoprotic acid solution to the
stoichiometric point. Determine the molar
concentration of the weak acid solution.
2.08 M
0.114 M
0.0831 M
0.00390 M
2.44 M
2)
For a weak acid (CH3COOH) that is
titrated with a strong base (NaOH), what species
(ions/molecules) are present in
the solution at the stoichiometric point?
CH3COO-
H2O
Na+
NaCl
HCl

A). To what volume should you dilute 121 mL of an 8.00 M CuCl2
solution so that 52.0 mL of the diluted solution contains 4.44 g
CuCl2?
B). Silver nitrate solutions are often used to plate silver onto
other metals. What is the maximum amount of silver (in grams) that
can be plated out of 5.1 L of an AgNO3 solution containing 3.4 % Ag
by mass? Assume that the density of the solution is 1.01 g/mL.
Express your answer...

a. You titrate 25.0 mL of 0.60 M NH3 with 0.60 M
HCl.
Calculate the pH of the solution after adding 5.00, 15.0, 22.0,
and 30.0 mL of the acid.
Ka = 5.6×10-10
pH(5.00 mL added) ------------------------------
pH(15.0 mL added)------------------------------
pH(22.0 mL added) ----------------------------
pH(30.0 mL added)----------------------------
b. itration of 27.9 mL of a solution of the weak base aniline,
C6H5NH2, requires 28.64 mL of
0.160 M HCl to reach the equivalence point.
C6H5NH2(aq) +
H3O+(aq) ⇆
C6H5NH3+(aq) +
H2O(ℓ)...

Part A
To what volume should you dilute 20 mL of a 12.0 M
H2SO4 solution to obtain a 0.130 M H2SO4 solution?
Express your answer using two significant figures.
Part A
Classify the following reactions:
HCl(aq)+NaOH(aq)→NaCl(aq)+H2O(l)
Ba(OH)2(aq)+ZnCl2(aq)→BaCl2(aq)+Zn(OH)2(s)
2AgNO3(aq)+Mg(s)→Mg(NO3)2(aq)+2Ag(s)
Drag the appropriate items to their respective bins.

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