Question

Calculate how many milliliters of 1 M NaOH will be needed to make 1 L of 0.1 M solution.

Calculate how many grams of potassium acid phthalate (KHP, FW = 204.2 g/mol) will react with about 25 ml of the 0.1 M NaOH solution. The reaction is as follows:

HKC8H4O4 + NaOH → H2O + NaKC8H4O4

Calculate how many mL of 1 M HCl is needed to make 1 L of 0.2 M HCl.

HCl + NaOH → H2O + NaCl

Answer #1

1) Let M and V be the initial molarity and initial volume and M' and V' be the final molarity and final volume of NaOH solution.

Hence, 100 mL of 1 M NaOH will be required to prepare 1 L of 0.1 M solution

2) As per balanced chemical reaction, 1 mole of KHP will react with 1 mole of NaOH.

Number of moles of NaOH

Number of moles of KHP = 0.0025

Mass of KHP

Hence, 0.51 g of KHP will react with 25 ml of 0.1 M NaOH

3) Let M and V be the initial molarity and initial volume and M' and V' be the final molarity and final volume of HCl solution.

Hence, 200 mL of 1 M HCl will be required to prepare 1 L of 0.1 M solution.

1. Answer the following question based on the reaction
below:
NaOH(aq) + KHP(s) ---> NaKp(aq) + H2O(l)
A 1.348g sample of impure KHP was titrated with a 0.0942 M
solution of NaOh. To completely react the KHP in the sample,
69.34mL of base was needed. KHP (potassium hydrogen phthalate,
204.23 g/mol)
a.)How many grams of KHP were in the unknown sample?
b.) What is the precentage of KHP in the unknown sample?

1). The volume of a stock 6 M NaOH solution required to prepare
250 mL of a 1 M NaOH solution.
2). The mass of potassium hydrogen phthalate (KHP) required to
react with 25 mL of a 1 M NaOH solution. The molecular weight of
KHP is 204.23 g/mol.
3). The amount of water required to dissolve the quantity of KHP
calculated in (b), given that the solubility of KHP is 10.2 grams
per liter.

1b. Calculate the exact molarity of a solution of NaOH if 55.00
mL of it is needed to titrate an amount of KHP that equals your
average mass (that you stated above). Average is 50.0 (4 pts)
2a. What is the average molarity for your standardized NaOH
solution?_______________ (1 pt) Average: .0075 M
2b. If 1.20 grams of impure solid KHP sample required 2.53 mL of
your standardized NaOH to reach the end point, what was the percent
KHP in...

Calculate how many milliliters of 0.100 M HCl solution is needed
to make a pH 4.34 solution with 2,2'-bipyridine, to 100.0 ml of
10.0 X 10-3 M of 2,2'-bipyridine.

(a) How many milliliters of 0.165 M HCl are needed to
neutralize completely 35.0 mL of 0.101 M
Ba(OH)2 solution?
________ ml
(b) How many milliliters of 2.50 M
H2SO4 are needed to neutralize 50.0 g of
NaOH?
_________ mL
(c) If 56.8 mL of BaCl2 solution is needed to
precipitate all the sulfate in a 544 mg sample of
Na2SO4 (forming BaSO4), what is
the molarity of the solution?
_________M
(d) If 47.5 mL of 0.250 M HCl solution...

(a) How many milliliters of 0.165 M HCl are needed to neutralize
completely 35.0 mL of 0.101 M Ba(OH)2 solution? ______ml
(b) How many milliliters of 3.50 M H2SO4 are needed to
neutralize 75.0 g of NaOH?
_______mL
(c) If 55.8 mL of BaCl2 solution is needed to precipitate all
the sulfate in a 544 mg sample of Na2SO4 (forming BaSO4), what is
the molarity of the solution?
________M
(d) If 47.5 mL of 0.375 M HCl solution is needed...

Calculate how many grams of NaHCO3 and mL of 1 M HCl is required
to make 80 mL of CO2 for the following reaction: NaHCO3 (s) + HCl
(aq) -> NaCl (aq)+ H2O (l)+ CO2 (g)
hint:remember that 1 M HCl contains 1 mole per liter.

How many grams of NaH2PO4 are needed to react with 30.66 mL of
0.260 M NaOH? NaH2PO4(s) + 2 NaOH(aq) → Na3PO4(aq) + 2 H2O(l)

How many grams of NaH2PO4 are needed to react with 32.94 mL of
0.280 M NaOH? NaH2PO4(s) + 2 NaOH(aq) Na3PO4(aq) + 2 H2O(l)

Answer the following for the reaction:
NiCl2(aq)+2NaOH(aq)→Ni(OH)2(s)+2NaCl(aq)
1.How many milliliters of 0.200M NaOH solution are needed to
react with 26.0 mL of a 0.420 M NiCl2 solution?
2.How many grams of Ni(OH)2 are produced from the reaction of
48.0 mL of a 1.80 M NaOH solution and excess NiCl2 ?
3.What is the molarity of 30.0 mL of a NiCl2 solution that
reacts completely with 11.3 mL of a 0.360 M NaOH solution?

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