The solubility of Mg(OH)₂ is measured and found to be 8.85×10-³ g/L. Use this information to calculate a Ksp value for magnesium hydroxide. Ksp' =

Q: Solid nickel(II) nitrate is slowly added to 75.0 mL of a 0.0690 M potassium carbonate solution. The…

A: The solubility product of salt is a constant at a given temperature irrespective of the source from…

Q: Calculate the maximum solubility of calcium fluoride, CaF2 in g/L when in the presence of 0.077 M…

A: Answer:- This question is answered by using the simple concept of calculation of solubility using…

Q: 125 mL of 0.315 mol/L sodium carbonate and 75.0 mL of 0.155 mol/L silver nitrate are mixed.  What is…

A: Molarity is defined as the number of moles of solute present in 1 L of the solution. M=nVn=M×V

Q: A solution contains 1.21x10-2 M silver acetate and 8.27x10-3 M lead nitrate. Solid sodium iodide is…

A: Given: Concentration of CH3COOAg = 0.0121 M Concentration of Pb(NO3)2 = 0.00827 M

Q: A saturated solution of iron(II) oxalate contains 0.0659 g FeC2O4 in 1.00 L of solution. What is the…

A:

Q: To determine the amount of Cl in an unknown sample, a NaCl sample was titrated with the titling…

A: Number of moles=massmolar mass From the given information, AgNO3 + NaCl → NaNO3 + AgCl Mass of…

Q: Considering the salt FeCl3, what is the mathematical relationship between its solubility product and…

A:

Q: A solution is prepared by adding 94.9 g of calcium nitrite, Ca(NO2)2, to 235. g of water. Determine…

A: Given :-  mass of calcium nitrite = 94.9 g mass of water                = 235 g Find out solution is…

Q: The solubility of silver sulfate, Ag, SO4, in water has been determined to be 8.00 g/L. What is the…

A: The concentration of SO42- ion in the solution, after the addition of Na2SO4, is 0.150 M. The…

Q: A solution contains 1.0 x 10- mol of KBr and 0.10 mol of KCI per liter. AGNO3 is gradually added to…

A: We have 10-5 mol of KBr, 0.1 mol of KCl in 1 liter solution. We have to predict which option will…

Q: Will strontium chloride (SrCl₂) precipitate when 300 mL of a 0.215 M solution of Sr(NO3)2 is added…

A: We know if Ionic product is more than solubility product then precipitate forms.If ionic product is…

Q: What is the solubility of PbF, in a solution that contains 0.0650 M Pb2+ ions? (Ksp of PbF, is 3.60…

A: Ksp of PbF2 = 3.60 * 10-8  [Pb2+] initially = 0.0650 M We need to determine the molar solubility.

Q: A solution contains 5.81x10-³ M magnesium nitrate and 8.75x10-3 M lead acetate. Solid potassium…

A: Addition of potassium fluoride to the solution containing magnesium nitrate and lead acetate causes…

Q: The solubility of magnesium fluoride, MGF2, in water is 1.5 x 10- g/L. What is the solubility (in…

A: Ksp is the solubility product constant, which explains the dissolution of a substance in an aqueous…

Q: The concentration of Cl- in a saturated solution of CuCl is 1.11*10^(-3)  mol/L at a certain…

A:

Q: Please don't provide handwritten solution ...

A: SELECTIVE PRECIPITATION: A selective precipitation reaction aims to separate two or more…

Q: Ksp for zinc hydroxide, Zn(OH)2, has a value 4.5 × 10-¹7 at 25 °C. Calculate the solubility of zinc…

A: Zn(OH)2 Ksp = 4.5 × 10-17  Zn(OH)2 <=> Zn2+(aq) + 2(OH-)(aq)  from here we can find solubility…

Q: 100 mL of 0.320 M AgNO3 is mixed with 100 mL of 0.160 M Na2SO4. How many grams of Ag2SO4 will…

A: Correct :c) 4.99 g Given that,  Volume of 0.320 M AgNO3 solution = 100 mL = 0.1 L Moles of AgNO3…

Q: Precipitation is the opposite of dissolution. Group of answer choices True False

A:

Q: The molar solubility of aluminum hydroxide is 0.0610 mol/L at a certain temperature. Calculate…

A: In this question, we have to find out the correct answer of given problem by the help of Solubility…

Q: Zn(OH)2 has a Ksp of 4.5 x 10-17. If you have a solution of Zn(OH)2 that has a hydroxide ion…

A: Given :  Ksp = 4.5 x 10-17  [OH-] = 4.6 x 10-6 mol/L

Q: a 66 lb child is preacribed 25 mg/kg/day of tetracycline three times a day. tetracycline is…

A: We know,1 lb = 0.453 kg

Q: A KClKCl solution containing 41 gg of KCl per 100.0 g of water is cooled from 70 ∘C to 0 ∘C. What…

A: A saturated solution is one in which a solvent has completely dissolved all of the solutes presents.…

Q: Solid lead acetate is slowly added to 75.0 mL of a 0.0317 M potassium hydroxide solution. The…

A: 2KOH(s) + Pb(Ac)2(aq) ------> 2KAc(aq) + Pb(OH)2 (s) So, Pb(OH)2 is the precipitate of the…

Q: You have a sample of cheese that has rat poison in it. The active ingredient or the rat poison is…

A: A sample of cheese having Tl2SO4 as the active ingredient, whose percentage is to be determined.

Q: The solubility product of silver chromate (VI) at room temperature is 2.4 x 10^-12. Calculate the…

A: Given :  Ksp of silver chromate (Ag2CrO4) = 2.4 x 10-12

Q: The solubility of strontium fluoride, SrF2, in moles per liter, can be expressed in terms of the…

A: Solubility (S) :  Dissolution of substance per litre of solution is called solubility.  It is…

Q: Calcium citrate (Ca3(C6H5O7)2; MM = 498.46 g/mol), a common food preservative, has a Ksp of 1.12 ×…

A:

Q: The average normal concentration of Ca2+ in urine is 5.33 g/L. a) Calculate the concentration of…

A: Solubility is defined as the maximum amount of solute which is able to dissolve in a solvent. Solute…

Q: A solution contains 1.21x10-2 M potassium iodide and 8.27x10-3 M sodium bromide. Solid silver…

A: Given: Concentration of KI = 0.0121 M And concentration of NaBr = 0.00827 M

Q: molar mass of solute B is 101.103 g mol−1   A 100.5 g sample of solute B dissolved in 100 g of…

A: Given that,  A 100.5 g sample of solute B dissolved in 100 g of water is decreased from 85 °C to 35…

Q: When 25.0 mL of a 9.37×10-4 M manganese(II) sulfate solution is combined with 25.0 mL of a 6.72×10-4…

A: Given, When 25.0 mL of a 9.37×10-4 M manganese(II) sulfate solution is combined with 25.0 mL of a…

Q: The Ksp of beryllium hydroxide, Be(OH)₂, is 6.92 x 10-22. Calculate the solubility of this compound…

A: Ksp of Be(OH)2=6.92×10-22 Molar mass of Be(OH)2=43.026 g mol-1 Let solubility is S,then,

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.