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Stels [109]
3 years ago
9

A chemist is using a solution of HNO3 that has a pH of 3.75. What is [OH− ] for the solution?

Chemistry
2 answers:
snow_lady [41]3 years ago
8 0

Answer:

[OH-] = 5.62

n = -11

pOH = 10.25

Explanation: Just did it on edge

strojnjashka [21]3 years ago
7 0

Explanation:

It is known that pH is negative log of H^{+}. Also the relationship between pH and pOH is as follows.

                      pH + pOH = 14

                    3.75 + pOH = 14

                               pOH = 14 - 3.75

                                        = 10.25

Therefore,          pOH = -log [OH^{-}]

                          10.25 = -log [OH^{-}]

                     antilog 10.25 = - [OH^{-}]

                         [OH^{-}] = 5.6 \times 10^{-11}  

Thus, we can conclude that [OH^{-}] for the solution is 5.6 \times 10^{-11}.

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Which of the following concerning solutions is/are correct? 1. The solvent in a mixture of gases is generally considered to be t
pshichka [43]

Answer: 1. The solvent in a mixture of gases is generally considered to be the substance in greater amount. 2. The solid dissolved in a solution is known as the solute. 3. Solid solutions are called alloys.

Explanation:

A binary solution is made up of two components ,called as solute and another as solvent.

A solute is defined as the component which is present in smaller proportion. It can be in solid, liquid or gaseous phase. A solvent is defined as the component which is present in larger proportion in a solution. It can be in solid, liquid or gaseous phase.

Usually in liquid solutions , solid acts as solute and liquid acts as solvent. For example: In salt solution, salt is the solute and water is the solvent.

Solid solutions contains solid as solute and solid as solvent. These are called as alloys. For example : In brass, zinc is the solute and copper is the solvent.

4 0
3 years ago
Ok, I need helpies! .__.
yKpoI14uk [10]
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3 0
3 years ago
A 20.0-milliliter sample of 0.200 M K2CO3 solution is added to 30.0 milliliters of 0.400 M Ba(NO3)2 solution.
jenyasd209 [6]

Answer:

(B) 0.160 M

Explanation:

Considering:

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

Or,

Moles =Molarity \times {Volume\ of\ the\ solution}

Given :

For K_2CO_3 :

Molarity = 0.200 M

Volume = 20.0 mL

The conversion of mL to L is shown below:

1 mL = 10⁻³ L

Thus, volume = 20.0×10⁻³ L

Thus, moles of K_2CO_3 :

Moles=0.200 \times {20.0\times 10^{-3}}\ moles

Moles of K_2CO_3 = 0.004 moles

For Ba(NO_3)_2 :

Molarity = 0.400 M

Volume = 30.0 mL

The conversion of mL to L is shown below:

1 mL = 10⁻³ L

Thus, volume =30.0×10⁻³ L

Thus, moles of Ba(NO_3)_2 :

Moles=0.400\times {30.0\times 10^{-3}}\ moles

Moles of Ba(NO_3)_2  = 0.012 moles

According to the given reaction:

K_2CO_3_{(aq)}+Ba(NO_3)_2_{(aq)}\rightarrow BaCO_3_{(s)}+2KNO_3_{(aq)}

1 mole of potassium carbonate react with 1 mole of barium nitrate

0.004 moles potassium carbonate react with 0.004 mole of barium nitrate

Moles of barium nitrate  = 0.004 moles

Available moles of barium nitrate  =  0.012 moles

Limiting reagent is the one which is present in small amount. Thus, potassium carbonate is limiting reagent.

The formation of the product is governed by the limiting reagent. So,

1 mole of potassium carbonate gives 1 mole of barium carbonate

Also,

0.004 mole of potassium carbonate gives 0.004 mole of barium carbonate

Mole of barium carbonate = 0.004 moles

Also, consumed barium nitrate = 0.004 moles  (barium ions precipitate with carbonate ions)

Left over moles = 0.012 - 0.004 moles = 0.008 moles

Total volume = 20.0 + 30.0 mL = 50.0 mL = 0.05 L

So, Concentration = 0.008/0.05 M = 0.160 M

<u>(B) is correct.</u>

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