How many grams of La(IO3)3 will dissolve in 250.0 mL of 0.05 M NaIO3?

Q: What must be the concentration of Ag* to just start precipitating 0.10M PO?0.10 M CI

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Q: Calculate the molar solubility of Ag2 CrO4 in a solution that is 0.01 M in AgNO3.

A: We need to calculate the molar solubility of Ag2CrO4

Q: Calculate the molar solubility of CaF2 in a solution containing 0.250 M Ca(NO3)2.

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Q: Write the net ionic equations that explain why the following precipitate dissolves in 6M HCl:  MnS

A: The reactants given are  1) MnS  2) HCl The molecular reaction taking place will be  MnS (s) + HCl…

Q: NaI crystals are slowly added to a solution that is 0.100M Pb(NO3)2 and 0.100 M AgNO3. Which vill…

A: When the ionic product of any salt becomes equal or greater than its solubility product then the…

Q: What is the I- concentration just as AgCl begins to precipitate when 1.0M AgNO3 is slowly added to a…

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Q: What is the pH of a buffer made from 0.350 mol of HBrO (Ka = 2.5 × 10⁻⁹) and 0.070 mol of KBrO in…

A: Moles of HBro = 0.350 mole  Moles of KBrO = 0.070 mole  Volume of solution = 2.0 litre…

Q: 2. How many moles of Ag Br can dissolve in 1.0 L of 0.40M NH;? Kr [Ag(NH3)2] *= 1.7 x 107 Ksp(AgBr)…

A: Given: Kf [Ag(NH3)2]+ = 1.7×107 Ksp(AgBr) = 5.0×10-13 We have to calculate the number of moles of…

Q: 3. How many grams of Na,HPO, must be added to a solution of 500 mL of 0.25 M NaH,PO, in prder to…

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Q: Calculate the molar solubility of AgBr in 0.035 M NaBr (Ksp = 5 × 10–13).

A: AgBr (s) -------> Ag+1(aq)   +  Br-1 (aq)   Ksp = [Br-1] [Ag+1]    AgBr is in NaBr…

Q: What is the molar solubility of PbBr2 in 0.500 M KBr solution?

A: Given: Concentration of KBr solution = 0.500 M Known: Ksp for PbBr2 = 6.60×10-6

Q: Calculate the minimum concentration of ammonia needed in 1.0 L of solution to dissolve 3.0 × 10–3…

A: The formation of complexes are resulted from the dissociation of components in the solution and two…

Q: calculate the theoretical amount (in mL) of 0.100 M HCl required to precipitate Pb (MM=207.2) as…

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Q: What must be the concentration of Ag+ to just start precipitating 0.10 M PO, 3-?0.10 M CI-?

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Q: What is the formula of the Cu(II) species in the deep blue solution obtained with excess NH3! a. b.…

A: We are given questions on Reaction with Cu(II) with different ligands, we have to tell which complex…

Q: Determine the molar solubility of AgBr (Ksp = 5.40e-13) in 2.600 M S2O32- if the complex ion…

A: Since value of Kf is very large so it is assumed that all the Ag+ from AgBr is converted into the…

Q: Provide the correct reaction showing how FeCO3 has increased solubility when forming the complex ion…

A: Answer: Saturated solution is the solution that contains maximum amount of electrolyte in it at the…

Q: What you expect to observe on mixing 0.1M AgNO3 with 6M NH3. Will there be a color? Will bubbles…

A: Given: Reaction of 0.1 M silver nitrate with 6M ammonia solution To find: colour, will bubbles…

Q: Compare the solubility of silver carbonate in each of the following aqueous solutions: Clear All…

A: Common ion effect

Q: AgCI is more soluble in ?? solution? AgNO3 HCI NH3 KNO3

A: AgCl is weak electrolyte, it dissociates in little amount. In presence of the strong electrolyte…

Q: 3) Determine the molar solubility of chromium(I) hydroxide in a buffered solution with pH = 11.45.…

A: Given: Kf of Cr(OH)3=3×1029 Ksp of Cr(OH)4-=8×10-29 pH=11.45

Q: Determine the mass of sodium formate that must be dissolved in 250.0 cm3> of a 1.4 M solution of…

A: Given,1.4 M solution of formic acid to prepare a buffer solutionpH = 3.36.

Q: If 0.0490 g of AgIO3 dissolves per liter of solution, calculate the solubility-product constant.

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Q: What you expect to observe on mixing 0.1M Na2CO3 with HCl. Will there be a color? Will bubbles form?…

A: Balanced chemical equation: Na2CO3 (aq)  +  2HCl  (aq) ------>  2NaCl (aq)  +  H2O (l)  +  CO2…

Q: What is the molar solubility of BaSO4 in a 0.250-M solution of NaHSO4? Ka for HSO4− = 1.2 × 10–2.

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Q: 10.0 ml 0.010M Na;CO, is combined with 10.0 mL 0.010 M AGN0,. a. What, if anything, precipitates…

A: Given: Concentration of Na2CO3 = 0.010 M Volume of Na2CO3 solution = 10.0 mL = 0.010 L…

Q: A 0.170 mole quantity of NiCl, is added to a liter of 1.20 M NH, solution. What is the concentration…

A: Equilibrium constant (K) - equals to ratio of concentration of products and concentration of…

Q: A sample of 50.0 mL of 2.0 M HNO, (pKa=3.398) is titrated with 1.0 M KOH. Determine the pH after the…

A: We are authorized to answer three subparts at a time, since you have not mentioned which part you…

Q: 70

A: The ion product, Q for a compound is be expressed as : If Q > Ksp, the solution is…

Q: What you expect to observe on mixing 0.1M Zn(CO3)2 with 6M NH3. Will there be a color? Will bubbles…

A: The question is based on qualitative analysis. we have to describe the observations taking place.

Q: What is the pH of a buffer made from 0.220 mol of HCNO (Ka = 3.5 × 104) and 0.410 mol of NaCNO in…

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Q: A solution contains 0.250 M HA (Ka = 1.0 x 10-6) and 0.45 M NaA. What is the pH after 0.30 mole of…

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Q: Determine the molar solubility of Ag2SO4(s) in 0.500 L of a solution containing 19.50 g of K2SO4

A: Calculation number of moles of K2SO4:

Q: What you expect to observe on mixing 0.1M Na2CO3 with 3M H2SO4. Will there be a color? Will bubbles…

A: The reaction is based on qualitative analysis. we have to describe the observations.

Q: Consider the titration of 60.00 mL 0.120 M NaHCO3 with 0.250 M KOH. a. Determine the pH after…

A: Given,  The titration of 60.00 mL 0.120 M NaHCO3 with 0.250 M KOH.When added15.00mL KOH the pH of…

Q: A 26.0 ml sample of 0.317 M triethylamine, (C,H5);N, is titrated with 0.293 M hydrochloric acid. The…

A: Given: Concentration of weak base triethylamine (Assuming B) = 0.317 M

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

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Q: The solubility of which salts would be decreased by the addition of Na2CO3? Select all that apply.…

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Q: What you expect to observe on mixing 0.1M Na2CO3 with 6M NaOH. Will there be a color? Will bubbles…

A: Given: 0.1M solution of sodium carbonate is mixed with 6M sodium hydroxide To find: colour, bubbles…

Q: K; for the complex ion Ag(NH,),* is 1.7 x 10. K, for AgCl is 1.6 x 10-10. Calculate the molar…

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Q: Calculate the theoretical pH for the following solutions . A buffer prepared by 50.0 mL of 0.20 M…

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Q: What is the molar solubility of FeCl3 in water?

A: Given :-  The given salt is FeCl3  Molar solubility of FeCl3 in water = ?…

Q: How many grams of Pb(OH)2 will dissolve in 500 mL of a 0.050-M PbCl2 solution (Ksp = 1.2 × 10–15)?

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Q: A 0.130 mole quantity of NiCl, is added to a liter of 1.20 M NH, solution. What is the concentration…

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Q: write the reaction for the complex ion Cu(NH2)4SO4

A: This complex is actually written as: [Cu(NH2)4]SO4.H2O  The IUPAC name of this complex is :…

Q: What mass of AgBr will dissolve in 500.0 mL of 5.90 M NH₃? Ksp for AgBr is 5.0 × 10⁻¹³. For the…

A: The overall reaction for the solubility of AgBr in ammonia can be written as follows:

Q: What is the molar solubility of CaF2 in a solution containing 0.100 M NaF?

A: The concentration of Na+ and F- in NaF will be 0.1 M each. The dissociation reaction of CaF2 is as…

Q: . Calculate the pH of the 0.30 M NH3/ 0.36M NH4Cl buffer system. What is the pH after addition of…

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Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red. 

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.