Physics High School

A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution after the addition of 50.0 mL of KOH. The Kb of NH3 is 1.8 x 10-5, A) 4.74 B) 7.78 C) 7.05 D) 9.26 E) 10.34

Answers

Answer 1

The pH of the solution after the addition of 50.0 mL of KOH is 9.26

So, the correct answer is D.

The limiting reactant is the one that will be completely consumed in the reaction. In this case, NH₃ is the limiting reactant because it is present in a greater amount than the HNO₃.

This means that all of the HNO₃ will react with NH₃ and there will be some NH₃ left over.

To find the amount of NH₃ that will react, use stoichiometry:

1 mol HNO₃ reacts with 1 mol NH₃ 0.0050 mol HNO₃ reacts with 0.0050 mol NH₃

This means that 0.0100 mol - 0.0050 mol = 0.0050 mol of NH₃ remains after the reaction with HNO₃.

Now, find the concentration of NH₃ after the reaction:

0.0050 mol / 0.150 L = 0.033 M NH₃

Now, calculate the pOH of the solution:

pOH = -log(1.8 x 10⁻⁵) + log(0.033) = 4.74

Finally, calculate the pH of the solution:

pH = 14 - 4.74 = 9.26

Therefore, the answer is option D) 9.26.

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Answer 2

Option (c), The solution has a pH of 7.05. We are given the volume and the molarity of NH3 and HNO3 in the equation.

So, let's first calculate the moles of NH3 present in 100.0 mL of 0.10 M NH3.

The number of moles of NH3 in the solution will be: (100.0 mL / 1000 mL/L) × 0.10 M = 0.010 moles of NH3

Also, the number of moles of HNO3 in the solution will be the same because the two are reacted in a 1:1 ratio. Therefore, the number of moles of HNO3 in the solution will also be 0.010 mol. It is now time to calculate the concentration of the solution after the addition of 50.0 mL of 0.10 M KOH. Using the balanced chemical equation, KOH reacts with HNO3 in a 1:1 ratio as follows:

KOH(aq) + HNO3(aq) → KNO3(aq) + H2O(l)

Using the volume and molarity of KOH, we can calculate the number of moles of KOH in the solution as follows:(50.0 mL / 1000 mL/L) × 0.10 M = 0.0050 moles of KOH

Now we can determine the number of moles of HNO3 left in the solution by subtracting the number of moles of KOH from the original number of moles of HNO3:Number of moles of HNO3 = 0.010 - 0.0050 = 0.0050 mol

Finally, we can calculate the concentration of HNO3 in the solution using the new total volume of the solution. Since the total volume of the solution has doubled (from 100 mL to 200 mL), the molarity of the solution is halved:

Molarity of HNO3 = 0.0050 mol / 0.200 L = 0.025 M

The Kb value for NH3 is given in the question as 1.8 x 10-5. We can use this value and the concentration of NH3 to calculate the pKb as follows:

pKb = -log(Kb) = -log(1.8 x 10-5) = 4.74

The pH of the solution can now be calculated as follows:

pH = 14.00 - pOH = 14.00 - (pKb + log([NH3]/[NH4+])) = 14.00 - (4.74 + log(0.010/0.0050)) = 7.05

Therefore, the correct option is (C) 7.05.

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Related Questions

21.42 using cyclopentanone as your starting material and using any other reagents of your choice, propose an efficient synthesis for each of the following compounds

Answers

Cyclopentanone, C5H8O is a cyclic ketone and can be converted to various organic compounds with the help of different reagents. Thus, cyclopentanone can be used as a starting material to synthesize different organic compounds using various reagents and catalysts.

Here, efficient syntheses for three organic compounds using cyclopentanone as a starting material are given below:

1) 2-Methylcyclopentanone: It can be prepared by the reaction of cyclopentanone with isopropyl, magnesium bromide, followed by hydrolysis of the resulting product. This reaction is shown below:

2) Cyclopentylmethanol: It can be prepared by the reduction of cyclopentanone with sodium borohydride (NaBH4) in methanol. This reaction is shown below:

3) 2-Cyclopenten-1-one: It can be prepared by the dehydration of cyclopentanol, which can be prepared by the reduction of cyclopentanone with lithium aluminum hydride (LiAlH4). The dehydration of cyclopentanol can be carried out by the elimination of water molecule using an acid catalyst like H2SO4. The overall reaction is shown below.

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