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Tutor profile: Michael D.

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Michael D.
Chemistry PhD Student
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Questions

Subject: Physical Chemistry

TutorMe
Question:

Consider an ideal gas with a volume of V1. To what volume would you need to compress the gas to double its pressure? Express your answer in terms of V1.

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Michael D.
Answer:

First, recall the Ideal gas law, PV=nRT. We can use Boyle's law to answer this question, which is P1*V1=P2*V2 for an ideal gas where T and n are constant. If we want double the initial pressure (P1), we can write P2 as 2 * P1, then solve Boyle's law for V2. P1 * V1 = (2 * P1) * V2 (P1 * V1) / (2 * P1) = V2 Both P1 on the left side cancel out, leaving us with: (V1)/2 = V2

Subject: Chemistry

TutorMe
Question:

What is the molarity of a NaOH solution if 25.00 mL is required to completely neutralize 40.00 mL of a 1.50 M solution of HBr.

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Michael D.
Answer:

First, calculate the amount of H+ in solution before the NaOH was added. First step of this is to find the moles of HBr in the solution. (1.50 moles HBr/1 L) * (1 L/1000 mL) * 40.00 mL=0.06 moles HBr Because HBr is a strong acid it dissociates completely, so 0.06 moles of HBr produces 0.06 moles H+ (0.06 moles HBr = 0.06 moles H+). To completely neutralize this amount we have to add 0.06 moles of OH-. NaOH is a strong acid, so similarly 0.06 moles of NaOH produces 0.06 moles of OH- (0.06 moles OH- = 0.06 moles NaOH). Then we take that and the volume added (25) to find the concentration. (0.06 moles NaOH/25 mL) * (1000 mL / 1 L) = 2.4 M NaOH.

Subject: Basic Chemistry

TutorMe
Question:

Calculate the pH of the following solution: 0.01 M HCl

Inactive
Michael D.
Answer:

Because HCl is a strong acid, it dissociates completely. As a result, 0.01M HCl forms 0.01M H+ when dissolved in water. Because pH is equal to -log[H+], all we need is to solve -log[0.01]. Solving -log[0.001] with a calculator gives the pH value 4.61.

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