how to increase the ph from 4 to 5 of a 50ml solution with ka=1.0x10^-6
the pH and [s2-1 in a 0.21 M H2S solution. Assume Ka,-1.0x10-7. Ka,-1.0x10-19. Calculate pH [s2-] Calculate the pH of a 3.9x10 M solution of H2SO4 Need Help? Read it
the pH and [s2-1 in a 0.21 M H2S solution. Assume Ka,-1.0x10-7. Ka,-1.0x10-19. Calculate pH [s2-] Calculate the pH of a 3.9x10 M solution of H2SO4 Need Help? Read it
A titration is performed on 50mL of a 0.10 M solution of HN3 (Ka+1.9x10-5) with 0.10 M NaOH as the titrant. (a) What is the initial pH of the HN3 solution? (b) Calculate the pH of the solution after 25 ml of NaOH have been added (c) How many mL of NaOH are required to reach the equivalence point and what is the pH of the solution at the equivalence point.
if 50ml of a 0.440M acetic acid solution (CH3COOH) is mixed with 50ml of a 0.240M sodium acetate solution (NaOOCCH3) what is the pH of the final solution (Ka= 1.76*10^-5)
If 100ml of a 0.134 M solution of HNO2 and 0.056 LiNO2 is reacted with 50ml of a 0.100 M of KOH what is the resulting pH of the solution? Ka=4.6 x 10^-4
4.How many mL of 0.25M NaOH are required to neutralize 50mL of 0.4M H2SO4? 6.Define: oxidation, reduction, anode, cathode, electrochemical half-cell, and the Standard Electrode Potential. 7.You mix 500mL of 10-3M HCl with 500mL of 4 x 10-3M NaOH. What will be the pH of this solution? 8.If 50mL of 10-2M HCl is diluted to a final volume of 800mL with distilled water, what will be the pH?
15. Calculate the pH pf 1.0x10-10M HCI solution?
We're asked to find the pH of 50mL of .1 M of a weak acid (labeled HX), before we add any .1 M NaOH. The Ka is 1.5e-5. The pH I found was 4.00 (feel free to fact check me). Here's the part I need help with: -We are also asked to find the pH of the solution at the "endpoint". Not sure what this means. Do they mean equilibrium? If so, how would I calculate this? Thanks.
4. Calculate the pH of a solution that is 0.98 molar hydrofluoric acid (5) Ka (HF) = 6.8 x 10-4 Fill in the ICE table, (H1+), and pH.
Assuming that Ka is 1.85 *10-5 for acetic acid, calculate the pH at one-half the equivalence point and at the equivalence point for titration of 50mL of 0.100M acetic acid with 0.100M NaOH.
consider the titration of 50mL of 1.5 M HCOOH with .50 M NaOH. Ka= 1.8x10^-4 & Kb= 5.56x10^-11 what is the pH after 175mL of .50 M NaOH is added? what is the pH after 250mL of .50 M NaOH is added? please show steps (using ice table(s))