1. Titrate 15.00 mL of 0.256 M KHP solution requires 20.75 mL of an unknown NaOH solution to reach the equivalence point. What's the molarity of this unknown NaOH solution? Show your work.

a) In a NaOH and HCl titration lab: Suppose you add 40 ml of water instead of the 45 mL. How will this affect the calculations for the molarity of the HCI? (In this case, the molarity of HCl turned out to be 0.559 mol/L). While being specific. Explain why it will not matter or it will make the molarity high or it will make the molarity low. b) if you disregard the instructions to titrate until a persistent blue endpoint is reached and instead conclude the titration at the initial appearance of blue, describe the impact on the reported molarity of the CoC12 solution. Provide specific details and specify whether the reported molarity will be higher, lower, or remain unaffected.

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1,Titrate 15.00 mL of 0.256 M KHP solution requires 20.75 mL of an unknown NaOH solution to reach the equivalence point. What’s the molarity of this unknown NaOH solution? Show your work. Group of answer choices A, 0.185 B, 3.54 C, 1.85 D, 0.354   2,Titrate 1.2035g of solid KHP (KC8H5O4) requires 23.89 mL of an unknown NaOH solution to reach the equivalence point. What’s the molarity of this unknown NaOH solution? Show your work. Group of answer choices A, 0.147 B, 1.23 C, 0.231 D, 0.247

A 1.00 liter solution contains 0.23 M acetic acid and 0.30 M potassium acetate. If 0.150 moles of potassium hydroxide are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of potassium hydroxide.) +A. The number of moles of CH3COOH will remain the same. + B. The number of moles of CH3COO" will remain the same. C. The equilibrium concentration of H30* will remain the same. + D. The pH will remain the same. E. The ratio of [CH3COOH]/[CH;COO"] will decrease.

I know that the correct answer is a. But I just don't how to get to the correct answer.

Q6

A student performed three H2SO4 titrations in Part 2 using their 0.1048 M NaOH solution which they previously standardized in Part 1. They reported the following measurements:   Determination #1 Determination #2 Determination #3 Final NaOH Burette Reading 37.65 mL 28.35 mL 26.23 mL Initial NaOH Burette Reading 12.80 mL 4.05 mL 1.73 mL For every 1 mole of H2SO4, how many moles of NaOH are needed to reach equivalence in the titration? Report the integer number only (no units).

A 150 mL solution of NaOH is titrated with HI. Phenol red is the indicator, which is red at high pH values and yellow at low pH values. The indicator be [ Select ] when you first put it into your analyte, before any titrant is added. The indicator will be [ Select] at the endpoint. The indicator will be [Select] V if you overshoot the endpoint and add too much acid.

for pH titration lab! please help