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3 years ago

What does ACE stand for? What word did you add to the word cloud?

Chemistry

1 answer:

AVprozaik [17]3 years ago

6 0

Answer:

a person who excels at a particular sport or other activity.

Explanation:

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Enter the net ionic equation for this reaction. Express your answer as a net ionic equation. Identify all of the phases in your

Lisa [10]

Answer:

2H+(aq) + 2OH-(aq) → 2H2O(l)

Explanation:

Step 1: The balanced equation

2HCl(aq)+Ca(OH)2(aq) → 2H2O(l)+CaCl2(aq)

This equation is balanced, we do not have the change any coefficients.

Step 2: The netionic equation

The net ionic equation, for which spectator ions are omitted - remember that spectator ions are those ions located on both sides of the equation - will.

2H+(aq) + 2Cl-(aq) + Ca^2+(aq) + 2OH-(aq) → 2H2O(l) + Ca^2+(aq) + 2Cl-(aq)

After canceling those spectator ions in both side, look like this:

2H+(aq) + 2OH-(aq) → 2H2O(l)

6 0

3 years ago

What is it called when a consume wastes and dead organisms??????

8_murik_8 [283]

Decomposers and a few insects.

8 0

3 years ago

Calculate the mole fraction of the ionic species kcl in the solution.

sp2606 [1]

The question is incomplete, here is the complete question:

Calculate the mole fraction of the ionic species KCl in the solution A solution was prepared by dissolving 43.0 g of KCl in 225 g of water.

Answer: The mole fraction of KCl in the solution is 0.044

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

For water:

Given mass of water = 225 g

Molar mass of water = 18 g/mol

Putting values in equation 1, we get:

$\text{Moles of water}=\frac{225g}{18g/mol}=12.5mol$

For KCl:

Given mass of KCl = 43 g

Molar mass of KCl = 74.55 g/mol

Putting values in equation 1, we get:

$\text{Moles of KCl}=\frac{43g}{74.55g/mol}=0.577mol$

Mole fraction of a substance is given by:

$\chi_A=\frac{n_A}{n_A+n_B}$

For KCl:

Moles of KCl = 0.577 moles

Total moles = [0.577 + 12.5] = 13.077 moles

Putting values in above equation, we get:

$\chi_{(KCl)}=\frac{0.577}{13.077}=0.044$

Hence, the mole fraction of KCl in the solution is 0.044

8 0

3 years ago

What is the ph of a 7.5×10-3m oh- solution? ph=?

BlackZzzverrR [31]

We will assume complete dissociation.
Since we have the molarity of OH solution, we can calculate the p(OH) as follows:
p(OH) = -log(molarity of OH) = -log(7.5×10-3) = 2.1249

It is known that: p(H) + p(OH) = 14
Therefore, p(H) can be calculated as follows:
p(H) = 14 - p(OH) = 14 - 2.1249 = 11.875

7 0

4 years ago

What is the molarity of 225 mL solution containing 1.89g of K₂SO₃•8H₂O? * 2 points 3.77 x 10⁻³ M 6.44 x 10⁻¹ M 3.87 x 10⁻²M 2.78

SCORPION-xisa [38]

Answer:

2.78 x 10⁻² M

Explanation:

Step 1:

Data obtained from the question.

Volume = 225mL / 1000 = 0.225L

Mass of K₂SO₃•8H₂O = 1.89g

Molarity =..?

Step 2:

Determination of the number of mole of K₂SO₃•8H₂O

This is illustrated below:

Mass of K₂SO₃•8H₂O = 1.89g

Molar mass of K₂SO₃•8H₂O = (39x2) + 32 + (16x3) + 8[(2x1) + 16] = 78 + 32 + 48 + 8[18] = 302g/mol

Number of mole = Mass/Molar Mass

Number of mole of K₂SO₃•8H₂O = 1.89/302 = 6.26x10⁻² mole

Step 3:

Determination of the molarity.

Molarity = mole /Volume

Molarity = 6.26x10⁻² /0.225

Molarity = 2.78 x 10⁻² M

Therefore, the molarity of the solution is 2.78 x 10⁻² M

5 0

3 years ago