An analytical chemist is titrating 120.7 mL of a 0.08800 M  of methylamine (CH3 NH2 ) with a 0.5900 M solution of HIO3. The pKb of methylamine is 3.36. Calculate the ph of the base solution after the chemist has added 14.6 mL of the HIO3 solution to it. You may assume the final volume equals the initial volume plus the volume of HIO3 solution added. Round your answer to two decimal places.

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A: Here we  are required to find the pH of the solution.

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A:

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A:

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A: Here we required to find the pH of the solution.

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A:

Q: An analytical chemist is titrating 232.9 mL of a 0.2400M solution of cyanic acid (HCNO) with a 1.200…

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Q: b An analytical chemist is titrating 136.2 mL of a 0.7100M solution of methylamine (CH3NH2) with a…

A: Given: VCH3​NH2​​=136.2mL;[CH3​NH2​]=0.7100M;VHNO3​​=97.5mL;[H+]=0.4900MpKb​=3.36;pH=???Step 1:…

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A:

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A:

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A: Given;

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A:

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A: We have to calculate the pH of solution

Q: An analytical chemist is titrating 120.7 mL of a 0.08800 M  of methylamine (CH3 NH2 ) with a 0.5900…

A:

Q: An analytical chemist is titrating 181.5 mL of a 1.000M solution of cyanic acid (HCNO) with a…

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A:

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A:

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A: The question is based on the concept of titrations.   we are titrating a strong nitric acid with…

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A:

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A:

Q: An analytical chemist is titrating 208.8mL of a 0.7500M solution of methylamine CH3NH2 with a…

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A:

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.