What is the maximum concentration of Ni²+ that can be added to a 0.00920 M solution of Na2CO3 before a precipitate will form? (Ksp for NICO; is 1.30 x 10-7)

Q: Three drops of 0.20 M KI are added to 100.0 mL of a 0.010 M solution of AgNO3. Will a precipitate of…

A: Three drops of 0.20 M KI are added to 100.0 mL of a 0.010 M AgNO3 solution . The Ksp of AgI is 8.5…

Q: An acidic solution containing 0.019 M La³+ is treated with NaOH until La(OH)3 precipitates. At which…

A: Given concentration of La3+ = 0.019 M Ksp for La(OH)3 = 2×10-21 We have to calculate the pH at which…

Q: Predict whether a precipitate will form when you mix 175 mL of a 0.0055 M KCI solution with 145.0 mL…

A:

Q: f 27.5 mL of 1.63x10-9M of FeCl3 is added to 98.6mL of 2.58x10-9 M NaOH, will a precipitate of…

A: The question is based on the concept of solubility product principle. it  states that a weak…

Q: What is the maximum concentration of Ni²⁺ that can be added to a 0.00900 M solution of Na₂CO₃ before…

A:

Q: When 22.0 mL of a 1.02 × 10-4 M potassium hydroxide solution is combined with 22.0 mL of a 7.55 ×…

A: To determine whether a precipitate will form when 22.0mL of  1.02×10−4 M potassium hydroxide…

Q: If 18.0 mL of 6.09×104 M Pb(NO3)2 are added to 25.0 mL of 9.30×105 M NH Br, will solid PbBr2 (Ksp =…

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

Q: Will a precipitate form when 8.5 mL of 6.3 × 10-2 M lead(II) nitrate is added to 1.0 L of 1.2 × 10-3…

A:

Q: Lead (II) fluoride has a Ksp value of 2.7x10-8. What is the concentration of Pb2+ and F- ions in a…

A: The solubility product constant (Ksp) describes the equilibrium between a solid and its constituent…

Q: What is the maximum concentration of Ni²⁺ that can be added to a 0.00530 M solution of Na₂CO₃ before…

A: Given: Concentration of solution of Na₂CO₃ = 0.00530 M Ksp for NiCO₃ is 1.30 × 10⁻⁷ Solution of…

Q: 2.52 g of NaCl is added to 3.44 L of a 8.45 x 10-3 M solution of Pb(NO3)2. Will a precipitate of…

A: Given that,  Weight of NaCl = 2.52 g Moles of NaCl = 2.52 g/58.44 g/mol = 0.04312 mol Volume of…

Q: If 0.235 L of 1.48 x 10-2 M of Ca(NO3)2 is added to 0.688L of 3.25 x 0-2 M of Na2SO4, will a…

A: We have 0.235 L of 1.48 x 10-2  M of Ca(NO3)2 ,0.688L of 3.25 x 10-2 M of Na2SO4 .Ksp as 9.1*10-6 .…

Q: The solubility-product constant for barium permanganate, Ba(MnO4)2, is 2.5 * 10-10. Assume that…

A: Given, Ksp=2.5×10-10 [Ba2+][MnO4-]2=2.5×10-10[Ba2+]=2.0×10-8

Q: Determine is a precipitate  of Ca3(PO4)2 will form when 100.0 mL of a 2.0x10-6M solution of CaCl2 is…

A: Ionic product  = [Ca2+]3[PO43-]2 Precipitation will form when     KSP < ionic product

Q: 500 mL of 0.12 M Pb(NO3)2 were mixed with 200 mL of 0.14 M KBr. Ksp for PbBr2 = 6.6x10-8. How many…

A: The objective of the question is to determine the mass of .It is given that,The volume of  is .The…

Q: Solid Na, SO4 is added slowly to a solution that is 0.76M in Pb(NO3), and 0.55M Ba (NO3)2. In what…

A:

Q: How many grams of sodium sulfate can be added to 310. mL of 1.5 x 10-3 M barium chloride before a…

A: The solubility reaction of BaSO4 is given by  => BaSO4 (s) ----> Ba2+ (aq) + SO42- (aq)  Hence…

Q: Ksp for Ca(OH)2 is 1.3 x 10-6.  A solution has a concentration of 0.0020 M Ca2+ and 0.0040 M OH-.…

A: The solubility product constant for Ca(OH)2 is = 1.3 x 10-6 The concentration of calcium ion is =…

Q: In which solution will 0.0020 M AgNO3 form a precipitate? a 7.1x10-7 M NaBr (Ksp of AgBr=5.0x10-13)…

A: Data given:  Concentration of AgNO3 = 0.0020 M  a. Concentration of NaBr = 7.1×10–7 M (Ksp of AgBr =…

Q: What is the molar solubility of strontium carbonate in a solution that contains 0.19-M SrCl2?…

A: Data given: Concentration of SrCl2 = 0.19 M Ksp (SrCO3) = 9.3 × 10–10

Q: Suppose 100 mL of 2.0 × 10–4 M Fe(NO3)3is added to 100 mL of 2.0 ×10–5 M KIO3. What is Qsp value?…

A: when Qsp < Ksp and then compound does not precipitated. For precipitation, Qsp > Ksp

Q: The solubility product of Mg(OH)2 is 1.2x10-11. Predict whether a precipitate will be formed or not…

A: The volume of 0.01 M MgCl2 added = 20.0 mL The volume of 1x10-3 M NaOH solution added= 30.0 mL We…

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.