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3 years ago

(science)

Chemistry

2 answers:

emmainna [20.7K]3 years ago

4 0

The answer is simulus check baby girl

____ [38]3 years ago

3 0

Heroin is an opioid drug so the same as stimulant

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A solution of CuSO4 is labelled 0.01 M. How much CuSO4 in grams, must be used to make 1 liter of solution?

Mkey [24]

Correct answer: C) 1.6 g

Molarity is the moles of solute present per liter solution.

The given molarity of the solution is 0.01 M.

Volume of the solution = 1 L

Calculating the moles from molarity and volume:

$Moles of CuSO_{4} = 0.01 \frac{mol}{L} * 1 L = 0.01 mol CuSO_{4}$

Converting moles to mass of copper sulfate:

$0.01 mol CuSO_{4} * \frac{159.61 g CuSO_{4}}{1 mol CuSO_{4}} = 1.6 g CuSO_{4}$

4 0

4 years ago

Read 2 more answers

Mg(OH)2 is a sparingly soluble salt with a solubility product, Ksp, of 5.61×10−11. It is used to control the pH and provide nutr

Solnce55 [7]

Answer:

The ration of the molar solubility is 165068.49.

Explanation:

The solubility reaction of the magnesium hydroxide in the pure water is as follows.

$Mg(OH)_{2}\Leftrightarrow Mg^{2+}(aq)+2(OH)^{-}(aq)$

$[Mg^{2+}][OH^{-}]$

Initial 0 0

Equili +S +2S

Final S 2S

$K_{sp}=[Mg^{2+}][OH^{-}]$

$5.61\times 10^{-11}=(S)(2S)^{2}$

$S=(\frac{5.61\times 10^{-11}}{4})^{1/3}=2.41\times 10^{-4}M$

Solubility of $Mg(OH)_{2}$ in 0.180 M NaOH is a follows.

$Mg(OH)_{2}\Leftrightarrow Mg^{2+}(aq)+2(OH)^{-}(aq)$

$[Mg^{2+}][OH^{-}]$

Initial 0 0

Equili +S +2S

Final S 2S+0.180M

$K_{sp}=[Mg^{2+}][OH^{-}]$

$5.61\times 10^{-11}=(S)(2S+0.180)^{2}$

$S=1.46\times 10^{-9}M$

$Ratio\,of\,solubility=\frac{2.41\times 10^{-4}}{1.46\times 10^{-9}}=165068.49$

Therefore, The ration of the molar solubility is 165068.49.

4 0

3 years ago

What is the percent by weight (w/w%) of sugar in soda? Assume the average mass of sugar in soda is 23.0 g and the total mass is

Nina [5.8K]

The percent by weight (w/w%) of sugar in soda : 6.216%

<h3>Further explanation</h3>

Given

mass of sugar = 23 g

total mass = 370 g

Required

the percent weight

Solution

%weight = (mass of solute : mass of solution) x 100%

solute = sugar

solution = solvent + solute = water + sugar

percent weight of sugar in soda :

= (23 : 370) x 100%

= 6.216 %

7 0

3 years ago

what quantities will you need to measure to determine the specific heat of one of these liquids? (pivot)

olganol [36]

Answer:

Specific heat capacity is measured by determining how much heat energy is needed to raise one gram of a substance one degree Celsius. The specific heat capacity of water is 4.2 joules per gram per degree Celsius or 1 calorie per gram per degree Celsius

Explanation:

5 0

3 years ago

The heat of vaporization of water is 40.66 kJ/mol. How much heat is absorbed when 3.11 g of water boils at atmospheric pressure?

Roman55 [17]

Answer:

The amount of heat that is absorbed when 3.11 g of water boils at atmospheric pressure is 7.026 kJ.

Explanation:

A molar heat of vaporization of 40.66 kJ / mol means that 40.66 kJ of heat needs to be supplied to boil 1 mol of water at its normal boiling point.

To know the amount of heat that is absorbed when 3.11 g of water boils at atmospheric pressure, the number of moles represented by 3.11 g of water is necessary. Being:

H: 1 g/mole
O: 16 g/mole

the molar mass of water is:

H₂O= 2* 1 g/mole + 16 g/mole= 18 g/mole

So: if 18 grams of water are contained in 1 mole, 3.11 grams of water in how many moles are present?

$moles of water=\frac{3.11 grams*1 mole}{18 gramos}$

moles of water= 0.1728

Finally, the following rule of three can be applied: if to boil 1 mole of water at its boiling point it is necessary to supply 40.66 kJ of heat, to boil 0.1728 moles of water, how much heat is necessary to supply?

$heat=\frac{0.1728 moles*40.66 kJ}{1 mole}$

heat= 7.026 kJ

<u><em>The amount of heat that is absorbed when 3.11 g of water boils at atmospheric pressure is 7.026 kJ.</em></u>

7 0

3 years ago