A 0.050 M H2S solution contains 0.10 M NiCl2 and 0.35 M Hg(NO3)2. What pH is required to precipitate the maximum amount of HgS but none of the NiS?
A 0.050 M H2S solution contains 0.10 M NiCl2 and 0.35 M Hg(NO3)2. What pH is...
show work please
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was not given ksp
A 0.050 M H S solution contains 0.10 M NiCl, and 0.35 M Hg(NO3). What pH is required to precipitate the maximum amount of Hgs but none of the Nis?
A precipitate forms when a solution that is 0.10 M in Cu2+, Pb2+, and Ni2+ is saturated with H2S and adjusted to pH = 1. What sulfides are present in the precipitate? [H2S] = 0.10 M; for H2S, Ka1 ´ Ka2 = 1.1 ´ 10–24 Ksp: CuS = 8.5 ´ 10–45, PbS = 7.0 ´ 10–29, NiS = 3.0 ´ 10–21 (The answer is D, Could anyone explain it by steps?) A) CuS, PbS, and NiS B) PbS and NiS...
How many milliliters of 0.10 M sodium sulfide solution are required to precipitate all the nickel, as nickel (II) sulfide, from 25.0 mL of 0.20 M nickel (II) chloride solution? NiCl2 + Na2S - NIS + 2 Naci Numeric Response
Will NicOs precipitate from a solution that initially contains 0.0020 M NazCOs? 0.150 M NiCl2 and 1.20 M NH3? 9.
Will NicOs precipitate from a solution that initially contains 0.0020 M NazCOs? 0.150 M NiCl2 and 1.20 M NH3? 9.
Question 8 (2 points) An unknown solution is either 0.10 M LINO3 or 0.10 M Ba(NO3)2 or 0.10 M AgNO3. When 1 mL of 0.10 M KCl is added to the unknown, a white precipitate forms. What is the identity of the solution? a) AgNO3 b) LINO3 Oc) There is not enough information provided to identify the unknown d) Unknown could be either LINO3 or AgNO3 e) Ba(NO3)2
What is the pH of a buffered solution saturated with hydrogen sulfide ([H2S] = 0.10 M) at 25°C if PbS (s) is precipitated, leaving [Pb2+] = 1.0 × 10–7 M, without precipitating any MnS (s)? The original solution is 0.030 M in both Pb2+ (aq) and Mn2+ (aq). Ksp = 8.0 × 10–28 M2 for PbS (s),Ksp = 2.5 × 10–13 M2 for MnS (s), andSelect one:a. 0.03b. 2c. 0.4d. 7
2. What is the pH of a buffer containing 0.050 M NH3 and 0.050 M NHACI? 3. What is meant by buffer capacity? 4. Sketch a pH titration curve for the addition of 0.10 M HCl to 25.0 mL of a 0.10 M NH3 solution and indicate the "buffer zone". 4. Sketch a pH titration curve for the addition of 0.10 M HCl to 25.0 mL of a 0.10 M NHz solution and indicate the "buffer zone".
1) An aqueous solution contains 0.280 M NaHS and 0.128 M H2S. The pH of this solution is _____ 2) A buffer solution is 0.321 M in H2SO3 and 0.328 M in NaHSO3. If Ka for H2SO3 is 1.7×10-2, what is the pH of this buffer solution? pH = ________
Consider a galvanic cell that contains a Zn metal electrode and a 0.10 M Zn(NO3)2 solution in one half-cell and a Sn metal electrode and a 0.10 M Sn(NO3)2 solution in the other half-cell. If the measured Ecell value is +0.60 V and the Zn2+/Zn reduction potential is assumed to be -0.79 V, what is the Sn2+/Sn reduction potential? Show all work
What is the solubility of PbSO4 in a solution which originally was 0.050 M in Pb(NO3)2?