What is the pH at 90.00 mL of titrant in the titration of 50.00 mL of 0.400 M B (a generic base with Kp = (4.45x10^-10)) with 0.200M HNO3? Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10 Answer

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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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**Problem:**
What is the pH at 90.00 mL of titrant in the titration of 50.00 mL of 0.400 M B (a generic base with \( K_b = (4.45 \times 10^{-10}) \)) with 0.200 M HNO₃?

**Instructions:**

- Enter your answer in scientific notation with 3 significant figures.
- Do not include any units in your answer.
- Do not round any intermediate calculations.

**Note:** Your answer is assumed to be reduced to the highest power possible.

**Answer:**

Enter your answer in the form:
\[
\boxed{} \times 10^{\boxed{}}
\]
Transcribed Image Text:**Problem:** What is the pH at 90.00 mL of titrant in the titration of 50.00 mL of 0.400 M B (a generic base with \( K_b = (4.45 \times 10^{-10}) \)) with 0.200 M HNO₃? **Instructions:** - Enter your answer in scientific notation with 3 significant figures. - Do not include any units in your answer. - Do not round any intermediate calculations. **Note:** Your answer is assumed to be reduced to the highest power possible. **Answer:** Enter your answer in the form: \[ \boxed{} \times 10^{\boxed{}} \]
**Question:** What is the pH at 0.00 mL of titrant in the titration of 50.00 mL of 0.400 M B (a generic base with \( K_b = (4.28 \times 10^{-10}) \)) with 0.200 M \( \text{HNO}_3 \)?

**Instructions:**
- Enter your answer in scientific notation with 3 significant figures. Do not include any units in your answer.
- Do not round any intermediate calculations.

**Note:** Your answer is assumed to be reduced to the highest power possible.

**Your Answer:**

- [  ] x10^ [  ] 

(Boxes for inputting the base and exponent)
Transcribed Image Text:**Question:** What is the pH at 0.00 mL of titrant in the titration of 50.00 mL of 0.400 M B (a generic base with \( K_b = (4.28 \times 10^{-10}) \)) with 0.200 M \( \text{HNO}_3 \)? **Instructions:** - Enter your answer in scientific notation with 3 significant figures. Do not include any units in your answer. - Do not round any intermediate calculations. **Note:** Your answer is assumed to be reduced to the highest power possible. **Your Answer:** - [ ] x10^ [ ] (Boxes for inputting the base and exponent)
Expert Solution
Step 1

pH is the negative logarithm of hydrogen ion concentration.

Given data:

*Volume of base is 50.0 mL or 0.050 L.

*Volume of acid is 90.0 mL or 0.090 L.

*Molarity of base is 0.400 M.

*Molarity of acid is 0.200 M.

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