4 points What is the pH of 50.0 mL of a 0.045 M HBr solution? editorify
M Please select file(s) Select file(s) Q5.2 15 Points A 50.0 mL HBr (aq) solution is titrated with 25.78 mL of 0.110 M NaOH. What is the pH of the original solution? Show your work for full credit. How many mol of HBr are present in the sample solution? Enter your answer here mol HBr are present What is the pH of the original 50.0 mL of HBr solution? Enter your answer here pH Please select file(s) Select file(s) Q6...
A solution of 50.0 mL of 0.045 M Ca(NO,), is prepared. What volume (in mL) of 1.90 M NaOH must be added to the calcium nitrate solution to begin to precipitate solid Ca(OH), from the solution? K = 6.5 x 10 Hint: Solid Ca(OH), will begin to precipitate at the point where an equilibrium exists between the solid and aqueous ions. The volume of NaOH required, will be very small so you don't have to consider the dilution of the...
4. What is the pH of 2.00mL of 1.0 M HCI solution diluted to 50.0 mL? ( 2pts)
(10 marks) Calculate the pH after titrating 50.0 mL of a 0.100 M weak base solution (Kb = 7 x10-9) with: 0.200 M HBr to the equivalence point b. 50.0 mL of 0.200 M HBr
A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH after the addition of 19.0 mL of KOH. Express your answer numerically.
a 50.0 mL solution initially contains 0.300 M HCIO and 0.250 M KClO. what is the new pH after 1.0 mL of 2.0 M HBr is added ? Ka = 2.9 x 10^-8
4. 50.0 mL of 0.00200 M Ca2 solution buffer at pH 10.0 is titrated with 0.00200 M EDTA. At equivalence point (i.e. 50.0 mL EDTA has been added), what is the equilibrium concentration of Ca2, [Ca2], and what is the pCa? The formation constant of CaY, Kaa 5.0 x 1010, and α4 of EDTA at pH 10.0 is 0.35 4. 50.0 mL of 0.00200 M Ca2 solution buffer at pH 10.0 is titrated with 0.00200 M EDTA. At equivalence point...
A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH after the addition of 12.0 mL of KOH. Express your answer numerically. A 75.0-mL volume of 0.200 M NH3 (Kb=1.8×10−5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 13.0 mL of HNO3. Express your answer numerically. A 52.0-mL volume of 0.35 M CH3COOH (Ka=1.8×10−5) is titrated with 0.40 M NaOH. Calculate the pH after the addition of 33.0 mL...
4 points Determine the pH of a solution prepared by mixing 60.0 mL of 0.025 M HCl with 40.0 mL of 0.035 M HBr. answer in Question 7. I leo Mathull ditarit
A 50.0 mL solution of 0.140 M KOH is titrated with 0.280 M HC1. Calculate the pH of the solution after the addition of each of the given amounts of HCI 0.00 mL pH = 11.84 5.00 mL pH = 12.5 mL pH = 12.74 19.0 mL pH = 12.38 24.0 mL pH = 11.56 25.0 mL pH = 7 31.0mL pH = 1.7 A 50.0 mL solution of 0.140 M KOH is titrated with 0.280 M HC1. Calculate the...