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3 years ago

What is the [OH-] concentration of a solution with a pH of 5.5?

Chemistry

2 answers:

aleksley [76]3 years ago

5 0

Answer:

Explanation:

grandymaker [24]3 years ago

5 0

Answer:
C
Explanation:

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1.3

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What type of reactions release energy into the environment?

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Which of the following properties increases down the periodic table?

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3 years ago

(A tablet containing calcium carbonate and fillers with a mass of 1.631 g was dissolved in HCl. After the fillers were filtered

FrozenT [24]

Answer:

1) 0.825 grams is the mass of pure calcium carbonate product collected at the end of the experiment.

2) The mass % calcium carbonate in the tablet is 50.58%.

3) The mass % of calcium in calcium carbonate is 40.00 %.

4) Mass of calcium in a tablet is 0.33 g.

Explanation:

Mass of tablet = 1.631 g

Mass of the watch glass = 46.719 g

Mass of the watch glass + mass of calcium carbonate = 47.544 g.

Mass of calcium carbonate = 47.544 g - 46.719 g = 0.825 g

0.825 grams is the mass of pure calcium carbonate product collected at the end of the experiment.

Mass of calcium carbonate = 0.825 g

Percentage of calcium in tablet:

$\%=\frac{\text{Mass of calcium carbonate }}{\text{Mass of tablet}}\times 100$

$\%=\frac{0.825 g}{1.631 g}\times 100=50.58\%$

The mass % calcium carbonate in the tablet is 50.58%.

Percentage of calcium in calcium carbonate :

Molar mass of calcium carbonate = 100 g/mol

Atomic mass of calcium = 40 g/mol

Percentage of calcium in calcium carbonate :

$\%=\frac{\text{atomic mass of calcium}}{\text{Molar mass of}CaCO_3}\times 100$

$\%=\frac{40 g/mol}{100 g/mol}\times 100=40.00\%$

The mass % of calcium in calcium carbonate is 40.00 %.

Mass of calcium carbonate = 0.825 g

The mass % of calcium in calcium carbonate is 40.00 %.

Mass of calcium in a tablet : x

$40.00\%=\frac{\text{Mass of calcium in a tablet}}{0.825 g}\times 100$

$x=40.00\times \frac{0.825 g}{100}=0.33 g$

Mass of calcium in a tablet is 0.33 g.

3 0

3 years ago

A solution of NaCl ( aq ) is added slowly to a solution of lead nitrate, Pb ( NO 3 ) 2 ( aq ) , until no further precipitation o

3241004551 [841]

Answer:

The molarity of the $Pb(NO_3)_2$ solution = 0.1895 M

Explanation:

The mass of the $PbCl_2$ obtained = 10.55 g

Molar mass of $PbCl_2$ = 278.1 g/mol

The formula for the calculation of moles is shown below:

$moles = \frac{Mass\ taken}{Molar\ mass}$

Thus,

$Moles= \frac{10.55\ g}{278.1\ g/mol}$

$Moles_{PbCl_2}= 0.0379\ mol$

From the reaction:-

$Pb(NO_3)_2+2NaCl\rightarrow PbCl_2+2NaNO_3$

1 mole of $PbCl_2$ is produced from 1 mole of $Pb(NO_3)_2$

Also,

0.0379 mole of $PbCl_2$ is produced from 0.0379 mole of $Pb(NO_3)_2$

Mole of $Pb(NO_3)_2$ = 0.0379 mol

Volume = 200.0 mL = 0.2 L ( 1 mL = 0.001 L )

Molarity is defined as the number of moles present in one liter of the solution. It is basically the ratio of the moles of the solute to the liters of the solution.

The expression for the molarity, according to its definition is shown below as:

$Molarity=\frac{Moles\ of\ solute}{Volume\ of\ the\ solution}$

Thus,

$Molarity=\frac{0.0379}{0.2}\ M = 0.1895\ M$

<u>The molarity of the $Pb(NO_3)_2$ solution = 0.1895 M</u>

4 0

3 years ago