What is the pH of a 0.050 M HClO(aq) solution? Ka,HClO = 4.0 × 10−8 M.
The pH of a 1.50 M solution of HClO is 3.67. pH = pKa + log [base] / [acid] a. Calculate the Ka of HClO. b. Calculate the pH and the percent dissociation of a 0.0100 M solution of NaClO.
What is the approximate pH of a solution labeled 6 x 10^-5 M HBr?
You have 1.25 L of a 2.00 M solution of Hypochlorous acid, HClO to which you will add 1.5 M NaOH to adjust the pH. a) what is the pH of hte solution when 0.500 L of NaOH is added? b) How many mL of soldium hydroxide should be added to prepare the 7.00 pH buffer solution? c) If 75.0 mL of 1.5 M Ba(OH)2 is added to the buffer in part 'b' when it is starting at pH 7.00...
HClO is a weak acid (Ka=4.0×10−8) and so the salt NaClO acts as a weak base. What is the pH of a solution that is 0.014 M in NaClO at 25 °C?
1. Calculate the pH of a 0.0820 M solution of the acid HClO dissolved in water if Ka = 2.9x10-8. 2. Calculate the pH of a 0.4480 M solution of the base H2BO3-1 dissolved in water if Ka = 5.4x10-10 for H3BO3. 3. Calculate the pH of a solution containing the following compounds. (Note that these are concentrations before any reaction occurs). [NaH2PO4] 0.300 M [Na2HPO4] 0.840 M [KOH] 0.054 M 4. For the titration of 15.00 mL of 0.100...
Given: pH: 7.60 Concentration (M): 0.050 mL: 100mL Determine the Mass of Each Component Recall that buffers are formed from conjugate acid/base pairs. Using the information given about your assigned buffer, determine how much of each component (acid and base) you will need in order to prepare it in the lab. (This will require a system of equations because there are two “unknowns.”) Note: the conjugate acid in this case is H2PO4−, and the conjugate base is HPO42−. 1. Using...
Upload pictures of your graphs of pH vs. volume of base added for 0.050 M HX (strong acid) and 0.050 M HA (weak acid). Explain one similarity and one difference in the graphs.
Find the pH of a 0.050 M HCl solution. What would be the final pH if 50.0 mL of the 0.050 M HCl solution was diluted to 250. mL?
what is the ph of a 0.050 M solution of bromoacetic acid (BrCH2CO2H) with Ka=1.25x10^-3