Contentra/courses/_74259_1/cl/outlinefor..O 12 Steps of Gamble...m Veterans PortalO*NET OnLineEC Home | exploreheal..Scholarships - SAL.Patient3) In Part B of the experiment, what volume of ethyldiamine should you add?4) Why does adding 95% ethanol to the solution cause the compound to precipitate?pH pre-lab At1) What are you trying to calculate in part A? What are you trying to calculate in part B?2) HF is as weak, monoptoric acid with a Ka value of 6.6x104, Calculate the pH of a 0.25 M solution of this acid.3) If you made a buffer solution of HF and NaF, what would be the conjugate base?4) If the concentration of HF was 0.15 M and the concentration of NaF was 0,25 M. what would be the pH of the buffer?5) Write a reaction for the neutralization that would occur if you added a small amount of NaOH to the buffer solution desribed in question 3.Ca(OH)2 pre-lab At1) What are you using as an indicator in this lab? What color indicates the titration has reached completion?2) The molar solubility of Mg(OH)2 is 1.51 x 104 M. What volume 0f 0.002 M HCI would be required to titrate 100.0 mL of saturated Mg(OH)2?3) At the end point of the titration, what would happen if you added a few drops of NaOH? Why?Borax Pre-lab A1) As the temperature of the solution increases, does the Ksp increase or decrease?2) You will be using bromocresol green as the indicator for the titrations. What color will indicate the titration is complete?3) After titrating at several temperatures, you will make a plot in Excel with your data. What will go on the y axis? What will go on the x axis?4) If the equation for the line is y = 300x + 25, solve for the change in Enthalpy, change in Entropy, and change in Gibbs energy at 65 °C and incluchp

Weak acid and its salt will form buffer solution. Note: As per our company guideline we can answer…

2) HF is as weak, monoptoric acid with a Ka value of 6.6x104. Calculate the pH of a 0.25 M solution of this acid. 3) If you made a buffer solution of HF and NaF, what would be the conjugate base? 4) If the concentration of HF was 0.15 M and the concentration of NaF was 0.25 M, what would be the pH of the buffer?

2) HF is as weak, monoptoric acid with a Ka value of 6.6x104. Calculate the pH of a 0.25 M solution of this acid. 3) If you made a buffer solution of HF and NaF, what would be the conjugate base? 4) If the concentration of HF was 0.15 M and the concentration of NaF was 0.25 M, what would be the pH of the buffer?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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