A solution contains 0.250 M HA (К.-1.0 added to 1.00 L of this solution? 3. 10"...
A solution contains 0.250 MHA(Ka-1.0 x 106and 0.45 M NaA. What is the pH after 0.30 mole of HCl is added to 1.00 L of this solution? a. 7.44 .2.10 98.56 8.5.44 e.0.52
A 1.00 L solution contains 0.311 M HA (K3 = 3.04 - 10 ) and 0.796 M NaA. What is the pH of this solution? What is the pH if 0.318 L of 0.158 M KOH is added to the solution be? What is the pH if 0.636 L of 0.158 M KOH is added to the solution be?
A 1.00 L solution contains 0.326 M HA (Kg = 5.09 · 10-7. and 0.796 M NaA. What is the pH of this solution? What is the pH if 0.325 L of 0.219 M KOH is added to the solution be? What is the pH if 0.650 L of 0.219 M KOH is added to the solution be?
A 1.00 L solution contains 0.352 M HA (Ka = 4.66⋅10−64.66⋅10-6) and 0.758 M NaA. What is the pH of this solution? What is the pH if 0.310 L of 0.138 M KOH is added to the solution be? What is the pH if 0.620 L of 0.138 M KOH is added to the solution be?
A solution contains 0.352 M HA (Ka = 4.66⋅10−64.66⋅10-6) and 0.758 M NaA. What is the pH of this solution? What is the pH of this solution after 0.138 mol of HCl are added to 1.00 L of this solution? What is the pH of this solution after 0.276 mol of HCl are added to 1.00 L of this solution?
a) A solution contains 0.34 M of a weak acid HA (Ka = 2.0 x 10-7) and 0.17 M NaA. What is the pH after 0.05 M of HCl is added to this solution (assume no volume change) b) The pH of a solution containing 0.1 M of a weak acid HA is 6. Calculate Ka for this acid. Note the acids are unrelated for the two problem parts.
A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in LiF. Calculate the pH of the solution after the addition of 0.20 moles of solid LiOH. Assume no volume change upon the addition of base. The K a for HF is 3.5 × 10 -4. 3.63 3.46 4.24 2.85 4.41
What amount of HCl (at 1.0 M) gas must be added to 1.00 L of a buffer solution that contains [aceticacid]=2.0M and [acetate]=1.0M in order to produce a solution with pH= 3.75?
consider 100.0 ml of a buffer solution that contains [NaCH3COO]=[CH3COOH]=0.250 M a) what is the pH of this buffer? b) what should the ph of the buffer be after 50.0ml of water is added? explain c) wtite balanced net ionic for the reaction that occurs whrn 1.0 M HCl ir added to this buffer. d) after adding 10.0 ml of 1.0 M HCl what will the ph of the solution be? e) as more 1.0 M HCl is slowly added...
analytical chemistry A 1.00-L buffer solution was made with 0.150 M benzoic acid (HC7H3O2) and 0.250 M lithium benzoate (LiCHO2). How many mL of 1.00 M HCI should be added to obtain the new pH of 3.97? The K of benzoic acid is 6.5 x 10 0.83 x 10 ml 1.0 x 102mL 1.3 x 102mL 5.6 mL 9.8 mL