Question

A. You wish to prepare 198 grams of 10.3 %
Na_{3}PO_{4}. How many grams will need of sodium
phosphate and how many mL of water? Assume that the density of
water is 1.00 g / ml.

B. If 20.5 grams of an aqueous solution of cobalt(II) sulfate,
CoSO_{4}, contains 2.84 grams of cobalt(II) sulfate, what
is the percentage by mass of cobalt(II) sulfate in the
solution?

C. An aqueous solution of lead nitrate,
Pb(NO_{3})_{2}, contains 8.74 grams of lead nitrate
and 17.5 grams of water. What is the percentage by mass of lead
nitrate in the solution?

D. An aqueous solution is 1.00% by mass ethanol,
CH_{3}CH_{2}OH, and has a density of 0.996 g/mL.
What is the molarity of ethanol in the solution?

E. An aqueous solution is 22.0% by mass silver nitrate,
AgNO_{3}, and has a density of 1.22 g/mL. What is the
molarity of silver nitrate in the solution is?

F. An aqueous solution of 15.7 M ammonia, NH_{3}, has a
density of 0.892 g/mL. What is the percent by mass of
NH_{3} in the solution?

Answer #1

Following is my *Solution* to the
*First full
question* i.e. **Question: A)**

The *Answers* are found to
be the following:

- **Grams of
sodium phosphate (Na _{2}PO_{4}) = 20.39
gm**

**- Volume
(mL) of Water (i.e. H _{2}O) = 177.61 mL**

The *solution* to the above
*results,*
are discussed/explained below: (**i.e.** **in
image
format**):

** Correction:** In the
above

*Correct representation of Sodium
Phosphate is the following:*

*Sodium Phosphate* is
written as **Na _{3}PO_{4}**

A.) If 19.8 grams of an aqueous solution of cobalt(II) sulfate,
CoSO4, contains 2.00 grams of cobalt(II) sulfate, what is the
percentage by mass of cobalt(II) sulfate in the solution?
B.) An aqueous solution of aluminum chloride,
AlCl3, contains 3.57
grams of aluminum chloride and
17.5 grams of water.
The percentage by mass of aluminum chloride in the
solution is

You need to make an aqueous solution of 0.162 M
iron(II) sulfate for an experiment in lab, using a
250 mL volumetric flask. How much solid
iron(II) sulfate should you add?
___ grams
How many milliliters of an aqueous solution of
0.207 M copper(II) acetate is
needed to obtain 7.15 grams of the salt?
____mL
In the laboratory you dissolve 24.2 g of
lead nitrate in a volumetric flask and add water
to a total volume of 125 . mL....

You wish to prepare 185 grams of
3.43 % KF.
You will need ? grams of potassium fluoride and ?
mL of water.
Assume that the density of water is 1.00 g / ml.

1.
Vodka is advertised to be 80 proof, which is 40% by volume of
ethanol, C2H5OH. Assuming the density of the solution is 1.0 g/mL
and the density of ethanol is 0.789 g/mL. If the solution is at
25oC, what is the vapor pressure of water over the solution?
2. Calculate the molarity and molality of a solution of 50
grams of ethanol, C2H5OH (density = 0.789 g/mL) which is dissolved
in 200 mL of water (density = 1.00 g/mL).

A student makes a solution for analysis by mixing 5.97 grams of
Cu2SO4 into 377.3 grams of water. The density
of water at the temperature of the lab at the time the solution was
made is 0.9926 g/mL.
Calculate the molarity, molality, mole fraction, and mass percent
of the copper I sulfate.
Last person who tried to answer it answered it incorrectly
according to the quiz software.

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) How many grams of solid silver nitrate would you need to
prepare 150.0 mL of a 0.140 M AgNO3 solution? B) An experiment
calls for you to use 100 mL of 0.30 M HNO3 solution. All you have
available is a bottle of 3.8 M HNO3. How many milliliters of the
3.8 M HNO3 solution do you need to prepare the desired solution? C)
How many milliliters of water do you need to prepare the desired
solution?

1. Zinc metal and aqueous silver nitrate react according to the
equation: Zn(s) + 2AgNO3 ---> 2Ag (s) + Zn(NO3)2 When 5.00 g of
Zn reacts with an excess of AgNO3, (1.47x10^1) grams of silver are
produced. What is the percent yield?
2.What is the molarity of a solution made by dissolving
(7.54x10^0) g (assume 3 sig. figs.) of silver nitrate in water to
make (4.164x10^1) mL of solution?
3. What is the molarity of a solution made by diluting...

2.According to the following reaction, how many grams of
dinitrogen monoxide will be formed upon the complete reaction of
28.0 grams of ammonium nitrate?
3.According to the following reaction, how many grams of
hydrobromic acid are needed to form 25.4 grams of bromine
4For the following reaction, 3.96grams of chlorine gas are mixed
with excess bromine . The reaction yields 11.3 grams of bromine
monochloride . bromine ( g ) + chlorine ( g ) bromine monochloride
( g )...

What is the proper tool for measuring 75.0 mL of copper II
sulfate?
How many moles of copper II will be present in the solution if it
is 0.378M?
What is the proper tool for measuring 2.37g of copper II
nitrate?
How many moles of copper II are present in that amount of copper II
nitrate?
If you record 123.5 mL for a solution that has a mass of 176.1 g
what would be the density of the solution?

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