you want to separate Ni2+ and Mn2+ by precipitating the corresponding sulphides from each other. What pH value must you set so that one of the two metals is precipitated quantitatively (concentration in the solution less than/equal to 10/-5 mol/l) is precipitated while the other is still in solution?  Ksp (NiS): 10^-21, Kps (MnS): 10~15; Ks (H2S): 10 ~- 20, Saturation concentration of H2S in water: 0.1 mol/l

Q: If 316.0 mg of AgBr is completely dissolved in 144.0 mL of 0.12 M NH3, what is the equilibrium…

A: Given, The mass of the AgBr = 316.0 mg The concentration of ammonia (NH3) = 0.12 M The volume of the…

Q: Calculate the pH at the equivalence point in titrating 0.020 M solutions of each of the following…

A: (a) HClO4 is a strong acid and NaOH is a strong base. So, pH at equivalence  point = 7   HN3 and…

Q: (a) Calculate the pH of a buffer solution containing 0.40 mole of KF and 0.50 mol of HF in 1.50…

A: pH of buffer solution is calculated using Henderson–Hasselbalch equation, amount of strong acid HCl…

Q: 72. At 25°C, K, for PbBr, is equal to 8 x 10. If the salt is 80% dissociated, what is the solubility…

A: 72. For the dissociation of PbBr2 ,      PbBr2 (s)   <---->   Pb2+(aq)   +  2Br-(aq)     Ksp…

Q: A 45.0-mL sample of 0.66 M HA (Ka = 0.00084) is titrated with 0.67 M NAOH. What is the pH of %3D the…

A:

Q: The arsenic in a 1.22-g sample of a pesticide was converted toAsO43- by suitable chemical treatment.…

A: a). The oxidation state of As in AsO43- is +5. b). Silver arsenate is the name of  Ag3AsO4 by…

Q: Buffer solution is made by taking 0.404 moles of acid (Pka=5.83) & 0.468 moles of sodium acetate and…

A:

Q: A buffer solution is 0.467 M in HCIO and 0.321 M in NaCIO . If K, for HCIO is 3.5x10-8 , what is the…

A:

Q: A buffer solution contains 0.50 mol of hydrazoic acid (HN3) and 0.62 mol of sodium hydrazoate (NaN3)…

A: This problem is solved on basis of Handerson-Hassalbalch equation

Q: The solubility product of MgF, is 10-8.2. (A) What is the solubility of Mg* at equilibrium with…

A: Given: Ksp of MgF2 = 10-8.2 = 6.31 X 10-9 approx.

Q: Ammonia is a convenient buffer system in the slightly basic range. (a) What is the pH of a buffer…

A:

Q: If 2.13 g of CusO4 are dissolved in 9.0 × 102 mL of 0.30 M NH3, what are the concentrations of Cu2+,…

A: Moles of CuSO4 = Mass/Molar mass = 2.13g/(159.6g/mol) = 0.0133moles Volume = 9.0 ×102 mL = 0.9 L…

Q: Determine the pH during the titration of 72.9 mL of 0.465 M formic acid (K, = 1.8x10-4) by 0.465 M…

A: a. The chemical equation may be written as: Before KOH is added, the pH of the solution depends on…

Q: The nitrite ion is the conjugate base of the weak acid nitrous acid. The value of K, for NO,, is…

A:

Q: What is the equilibrium molar concentration of Cu+ in a solution prepared by adding 0.1558 mol of…

A: The reaction is as follows Cu+(aq) +     2CN-(aq)       [Cu(CN)2]-(aq)

Q: A frequently used buffer in biological systems, including IV fluids, is a phosphate buffered saline…

A: Step 1:

Q: 3.00 L of air sample is passed through 50.0 mL of 0.0116 M Ba (OH) 2 solution, and CO2 in the air,…

A: The substance concentration will be expressed in the term of ppm by the mathematical ratio between…

Q: If H+ ion is added to a reaction where: AgC2H3O2(s) + Cl-(aq) becomes AgCl(s) + C2H3O2-(aq), would…

A: The solubility of a species is defined as the maximum amount of a substance that is soluble in a…

Q: In which case will a precipitate form? (i) a 0.050 M MnCl2 solution with pH = 8.00 (Does Mn(OH)2…

A: Hi there! Since you have posted multiple questions, we will answer the first question for you.

Q: What is the Molar Mass (g/mol) of an unknown monoprotic weak acid if 648 mg of it requires 35.86 mL…

A:

Q: The solubility product constant for La(IO3)3 is 1.00×10-11 at 25 oC. How many grams of La(IO3)3 can…

A: Given, solubility product constant for La(IO3)3 is 1.00×10-11 0.100 M KIO3

Q: Which of the following pairs of solution would you use to prepare a buffer with pH = 7.45

A:

Q: A buffer solution contains 0.45 mol of hydrazoic acid (HN3) and 0.28 mol of sodium hydrazoate (NaN3)…

A: Given :  Ka = 1.9 x 10-5  Moles of HN3 = 0.45 mol  Moles of NaN3 = 0.28 mol  Volume = 8.60 L

Q: СОCL:* (ag) + 6 H:0 () — Со(H-0);2* (ag) + 4 Cl (ag) [C][D]" K= [A]"[B]* [COCl?] = 0.03346 M…

A: The given reaction is,                                CoCl42- (aq) + 6 H2O (l) -----> Co(H2O)62+…

Q: buffer solution contains 0.40 mol of arsenous acid (H3AsO3) and 0.87 mol of sodium dihydrogen…

A:

Q: A buffer solution is made that is 0.495 M in HNO₂ and 0.495 M in NaNO2. (1) If K, for HNO₂ is…

A: Given,  Molarity of HNO2 = 0.495 M Molarity of NaNO2 = 0.495 M Ka of HNO2 = 4.50 × 10-4 moles of KOH…

Q: Calculate the pH at the equivalence point in titrating 0.072 M solutions of each of the following…

A: (a) Hydrobromic acid (HBr): Reaction at equivalence point: HBr+NaOH→NaBr+H2​O pH=7.0 (neutral) (b)…

Q: Ammonia is a convenient buffer system in the slightly basic range. (a) What is the pH of a buffer…

A: pH is defined as the negative logarithm of hydrogen ion concentration.  It can be given as  pH=-log…

Q: A solution of phosphoric acid (H3PO4) with a known concentration of 0.250 M H3PO4 is titrated with a…

A: At third equivalence point, all the  H3PO4 molecule get converted to PO4-3 i.e complete…

Q: 17.72 Suppose that a 10-mL sample of a solution is to be tested for I ion by addition of 1 drop (0.2…

A: 1) Calculate the concentration of Pb2+ of Pb(NO3)2 in the mixture of solution. 2)As PbI2 is a…

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.