Calculate the concentration of ions in the following saturated solutions. (a) [I-] in AgI solution with [Ag+] = 9.0 × 10-9 M 4.0 M (b) [AI3+] in Al(OH)3 solution with [OH ] = 3.6 x 10-9 M 4.0

Q: Calculate K.

A: We know that  If the equilibrium constant is kc for forward reaction and the equilibrium constant is…

Q: 1. 18.0 g of zinc is added to 100. mL of 0.200M HBr.a) Will all of the zinc dissolve?b) What will be…

A: Solution stoichiometry involves the calculation of concentration of solutions in the given…

Q: A buffer solution is made that is 0.360 M in HNO2 and 0.360 M in KNO2. If K, for HNO2 is 4.50 ×…

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Q: If Kal for H2 CO3 is 4.20 x 10-, what is the pH of the buffer solution? pH = Write the net ionic…

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Q: 2. A buffer solution of volume 0.500 L contains 1.68 g NH3 and 4.05 g (NH);SOu. a) What is the pH of…

A: “Since you have asked multiple questions, we will solve the first question [Q2] for you. If you want…

Q: What is the molar solubility of AgBr in 0.25 M NH3 at 25 oC? Use the given information attached

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Q: Calculate the molar solubility of iron(II) hydroxide in an aqueous solution buffered at pH = 6.07.

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Q: Consider Al(OH)3(s) + 3H+(aq) ↔ Al 3+(aq) + 3 H2O(l) a. Calculate K for this reaction. b. Calculate…

A: Given data :  pH of acid = 4.0  a)To get the K value we will devide concentration of products to the…

Q: Calculate the equilibrium concentration of Zn2+ in a 0.30-M solution of Zn(CN)4 2−.

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Q: A buffer solution with a pH of 3.86 is prepared with 0.50 M formic acid and M sodium formate. The K,…

A: The formula of pH of a buffer solution is: pH=pKa+log[Salt][Acid]

Q: gravimetric analysis

A: In gravimetric analysis we add a Precipitating reagent into the analyte to make ppt then filter dry…

Q: If you put a pure copper penny in an aqueous solution of AgNO3, which of the following will happen?

A: On putting a pure copper penny in an aqueous solution of AgNO3, a reaction will occur.

Q: The formation constant* of [M(CN)4]²- is 7.70 × 1016, where M is a generic metal. A 0.150 mole…

A: Given: The formation constant of [M(CN)4]2- is 7.70×1016. The number of moles of M(NO3)2 or M2+…

Q: Compare the molar solubility of Mg(OH)2 in pure water with that in a solution buffered at pH 9.00.

A: The dissociation of Mg(OH)2 is Mg(OH)2 s⇋Mg2+ aq+ 2OH- aq. For pure water: Ksp = (s)(2s)2 =…

Q: A buffer solution is made that is 0.401 M in HCN and 0.401 M in KCN. If Ka for HCN is 4.00 x 10 0,…

A: A buffer solution is made of a weak acid ie. Hydrocyanic acid (HCN) and potassium cyanide (KCN). pH…

Q: The formation constant* of [[M(CN),]- is 5.30 x 1018, where M is a generic metal. A 0.140 mole…

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Q: Which of the following salts will the solubility in water depends on pH of the solution: AgF,…

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Q: The formation constant* of [M(CN)6]t- is 2.50 × 10'7, where M is a generic metal. A 0.180 mole…

A: We have to calculate the concentration of M2+

Q: Calculate the concentration of free Zn2+ ion at equilibrium when 1.58x10-2 mol zinc sulfate is added…

A: Each zinc sulfate, ZnSO4 produces 1 Zn2+(aq) ion Hence moles of Zn2+(aq) ion added to 1.00 L…

Q: Calculate the pH of the solution produced when 20.o mL of o.125 M HCI are mixed with 50 mL of each…

A: Given :             Volume of HCl = 20.0 mL            Molarity of HCl = 0.125 M            Volume…

Q: Calculate the molar solubility of BaSO4 in a solution containing 1.0 M SO4 -2 ions

A: Given , BaSO4 [SO42-]= 1.0 M

Q: B.) What is the approximate concentration of free Zn2+ ion at equilibrium when 1.00x10-2 mol zinc…

A: The equilibrium constant for the formation of a complex ion is called the formation constant , Kf.…

Q: when AgCl dissolves in ammonia solution , which is the principle cation present in the solution?

A: Added ammonia to silver chloride (s) dissolves the solid by displaced chloride ions with ammonia…

Q: What is the molar solubility of PbBr2 in a 0.500 M Pb(NO3)2 solution?

A: Ksp of PbBr2 = 6.60 x 10-6 Pb(NO3)2 ----> Pb+2       +          2NO3- PbBr2 ----> Pb+2 + 2Br-…

Q: How many ions exist in the in the complex Ka[Fe(Ox)a] oa. 4 ions Ob. O b. 5 ions Oc. 6 ions d. 7…

A: Since you asked multiple questions so as per Q&A guidelines of portal I solve first question…

Q: What are the concentrations of Ag+, CN–, and Ag(CN)2 − in a saturated solution of AgCN?

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Q: Calculate the concentration of PO4^3- when Ag3PO4 starts to precipitate from a solution that is…

A: The solubility product Ksp for Ag3PO4 = 1.8 x 10-18 Ksp expression for the Ag3PO4 , Ksp = [Ag+]3…

Q: [20] ml of [4] M HC2H3O2 is titrated with 2.25 M sodium hydroxide. Ka for HC2H3O2 is 1.8 x 10-5 d.…

A: Given: Concentration of HC2H3O2 (assuming it HA) = 4 M The volume of HA taken = 20 mL And the…

Q: A buffer solution is 0.100 M in both HC7H5O2 and LIC7H5O2 and has a pH of 4.19. Which of the…

A: The buffer solution is that can resist the small change in PH  by the addition of acid or base.

Q: The pH value for 0.01 M potassium cyanide is 7x10-10 respectively -(when Kw & Ka are 1x10-14 & ---

A: Given: Kw=1×10-14Ka=7×10-10 KCN(potassium cyanide) is a salt of a strong base (KOH) and a weak acid…

Q: a) Calculate the K for this reaction: 2Fe ag) + Pd* + Pd*2, (aq) * 2Fe*3, + Pd (aq) b) Calculate the…

A: Interpretation : We have to calculate K and equilibrium concentration of all the species.

Q: Fe(OH)2(s) + Pb(OH)3-(aq) ---> Fe(OH)3(s) + Pb(s) in basic solution

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Q: - The concentration of ammonia (17.031 g/mol) can be determined through back titration. After…

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Q: Agl has very low solubility in water. If the Kf of [Ag(CN)2) is 1.0 x 1021 and sodium cyanide is…

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Q: Calculate the pH of the following two buffer solutions: (a)2.0 MCH3COONa/2.0 M CH3COOH, (b) 0.20 M…

A: The pH of a acidic buffer can be calculated as follows: pH=pKa+logSaltAcidwhere Ka is the…

Q: A 29.5 mL sample of 0.258 M ethylamine, C2H5NH2, is titrated with 0.340 M hydrochloric acid. After…

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Q: Calculate the concentration of ions in the following saturated solutions: (a) [I] in AgI solution…

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Q: what is the pH of this buffer solution?

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Q: 16.72 Calculate the molar concentration of OH in a 0.724 M solu- tion of hypobromite ion (BrO"; K, =…

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Q: Calculate the molar solubility of BaSO4 in a solution in which H3O+ is 0.5 M

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Q: Calculate the molar solubility of Ni(OH)2 when buffered atpH (a) 8.0, (b) 10.0, (c) 12.0.

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Q: The pH of buffer solution that has Ka = 6.23 x 105 and 5a, = 3a, is: а. 4.43 b. 4.03 С. 4.38 d. 3.98…

A: pH = d.  3.98

Q: What is the concentration of Ag* (aq) ion in 0.010 M AgNO, that is also 1.00 M NH,? K, for Ag(NH3)2*…

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Q: A buffer solution is 0.402 M in H2CO3 and 0.314 M in KHCO3. If Kal for H2CO3  is 4.2 X 10 -7 , what…

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Q: The titration of Na,Se with HCI has the following qualitative profile. pH E F V2 mL HCI (a) Identify…

A: Point A : Na2Se  Point B : Na2Se + NaHSe  Point C : NaHSe ( first equivalence point)

Q: 4. When the above-mentioned indicators are dropped into the 0.1 M NH3, what will the color of…

A: The indicator is the species that is used to identify the acid and base on the basis of its pH range…

Q: A buffer solution is 0.441 M in HF and 0.245 M in NaF . If Ka for HF is 7.2×10-4 , what is the pH of…

A: Given, concentration of HF , [HF] = 0.441 M            concentration of NaF, [NaF] = 0.245 M…

Precipitation Titration

Precipitation analysis is used to analyze drugs, and to measure the salt content in food and beverages. It is an important concept from the examination point of view many practical questions are asked on the topic. This topic is significant in the professional exams for both undergraduate and graduate courses, especially for