A solution contains 3.25x10-5 M Ca2+ and 7.25 x10-5 M CO3²-. Will a precipitate form in the solution? CaCo3(s)= Ca2+(aq) + CO3²-(aq) Ksp = 3.4x10-9 No, because QK No, because Q>K

Q: 44. In which solution will 0.0010 M AgNO3 form a precipitate? a. 2.0x10-7M NaCl (Ksp of…

A: For the precipitation to occur: [Ag+][X-] > Ksp

Q: The Ksp for CaF2 is 3.9 * 10-11 at 25 °C. Assuming equilibrium is established between solid and…

A: In order to calculate the solubility we first write down the given data: Ksp= 3.9*10-11. Solubility…

Q: In which solution will 0.00015 M BaCl2 form a precipitate?   7.0x10-7M H2SO4 (Ksp of…

A: Interpretation - To determine in which solution formation of precipitate formation take place -…

Q: The solubility-product constant for Ce(IO3)3 is 3.2x10^-10. What is the Ce3+ concentration in a…

A: Given: Concentration of Ce3+ = 0.0450 M Volume of Ce3+ solution = 50.0 mL = 0.050 L  Concentration…

Q: A solution contains three anions with the following concentrations: 0.20 M CrO42 - , 0.10 M CO32 - ,…

A: Given: The concentration of CrO42- in the solution is 0.20 M The concentration of CO32- in the…

Q: Will a precipitate of magnesium fluoride form when 300.0 mL of 1.1 x 10-3 M MgCl2 are added to 500.0…

A:

Q: A solution is prepared by mixing 50.0 mL of 0.50 M CaCl2 with 50.0 mL of 0.50 M CoCl2. When Na2CO3…

A: Given,  Molarity of CaCl2 = 0.50 M  Volume of CaCl2 = 50.0 mL Molarity of CoCl2 = 0.50 M  Volume of…

Q: SrF2(s) ⇄ Sr2+(aq) + 2F-(aq)      Ksp = 2.0 x 10-10 25.0 mL of 0.160 M Sr(NO3)2 is mixed with 75.0…

A: Answer = The correct option is (b) 8.2×10-5 M Solution -

Q: Will a precipitate form when 3.0 mL of 0.000150 M FeBr₃ is mixed with 1.0 mL of .00030 M AgNO₃ in…

A: We will first find Qsp , then compare it with Ksp to check whether precipitate will form or not.

Q: Exactly 500 mL of 0.058 M MgCl2 are mixed with exactly 300 ml of 0.0019 M K2CO3. Will a precipitate…

A:

Q: A solution contains 6.71×10-3 M barium acetate and  1.21×10-2 M calcium nitrate.  Solid potassium…

A: Given information: 6.71×10-3 M barium acetate 1.21×10-2 M calcium nitrate.    KSP for BaF2 is…

Q: Will Ag2Cr207 precipitate when 150.0 mL of 1.2 × 103 M AGNO3 are added to 50.0 mL of 1.9 x 10-2 M…

A: Solubility product   It is the product of concentration term raised to the power of their…

Q: The Ksp for BaF2 is 2.4 × 10–5. When 10 mL of 0.01 M NaF is mixed with 10 mL of 0.01 M BaNO3, will a…

A: The solubility product constant (Ksp) represents the solubility of products at equilibrium for…

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: A solution contains 2.0 x10-4 M Ag+(aq) and1.5 x 10-3 M Pb2 + (aq). If NaI is added  , wi l l…

A:

Q: following mixture. Ksp for BaSO4 = 1.08 × 10−10, Ksp for SrSO4 = 3.44 × 10−7 I. Add 650 mL of…

A:

Q: If you make a solution where the concentration of Pb2+ = 0.050 M and the concentration of Br- =…

A: Given: Concentration of Pb2+ = 0.050 M Concentration of Br- = 0.0065 M Ksp of PbBr2 at 25oC =…

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

A:

Q: 0.013 g Cu (ii) ion and 0.04 g Pb (ii) ion are to be separated in 1 000 mL water using sodium…

A: Given the Ksp of Cu(OH)2 = 2.2*10-20  Ksp of Pb(OH)2 = 1.2*10-15  Ksp of Pb(OH)2 >> Ksp 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: A solution has ​[Ag^+] = ​[Pb^2+] = ​[Hg2^2+] = 0.0040 M, what’s the concentration of Cl- to…

A: Given: ​[Ag^+] = ​[Pb^2+] = ​[Hg2^2+] = 0.0040 M Ksp (AgCl) = 1.8 × 10^-10 Ksp (PbCl2) = 1.2 × 10^-5…

Q: Will a precipitate form when 100.0 mL of 3.8x10-4 M Mg(NO3)2 is added to 100.0 mL of 2.6x10-4 M…

A: The solubility product constant (Ksp) represents the solubility of products at equilibrium for…

Q: Given: Will a precipitate form when 0.100 L of a solution containing 0.55 M barium nitrate is added…

A: In order to know whether precipitate is formed or not follow the below mentioned steps: 1) Calculate…

Q: Will a precipitate form when 0.96g of (NH4)2CO3 is mixed with 0.020g of CaBr2 in 20 L of solution?…

A: Since moles of  (NH4)2CO3 = mass / molar mass molar mass of (NH4)2CO3 = 96 g/mol and molar mass of…

Q: For PBCI 2 (K sp = 2.4 x 10-4), will a precipitate of PbCl , form when 0.10 L of 3.0 x 10 -2 M Pb(NO…

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

Q: You prepare a solution by mixing 400.0 mL of 1 x 10-4 M Mg(NO3)2  and 500.0 mL of 1.00 x 10-4 M NaF.…

A: Solubility product for MgF2 can be writte as Ksp =Mg2+F-2 Now, to determine weather precipitate…

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: The ksp of NiCO3 is 6.6x10-9 @ a certain temperature. If 5.0 mL of 1.7x10-5M Ni2+ ions were added to…

A: Given,  The ksp of NiCO3 is 6.6x10-9 . If 5.0 mL of1.7x10-5M Ni2+ ions were added to 5.0 mL of…

Q: solid sodium sulfate, Na2SO4, is added slowly to a solution that is 1.0x10^-4 in both Ba2+ and Pb2+…

A:

Q: At 25 °C, for Lead (II) sulphate (PbSO4), Ksp = 2.53×10-8 and for Barium sulphate (BaSO4) Ksp =…

A: Solution:

Q: Will a precipitate form in a solution whose concentrations of ions after mixing are the following:…

A: We can decide whether a precipitate will form or not on the bases of the Q and Ksp value Q<KSP =…

Q: A solution prepared in the lab contains 3.5 x 10-4 M Sr2 and 0.0010 M F-. Will a precipitate form?…

A: Given:[Sr2+] = 3.5 x 10-4 M [F-] = 0.0010 M Dissociation reaction of SrF2: SrF2(s)  ⇔   Sr2+(aq)  +…

Q: 75.0-mL sample of 0.003 M AgNO3 is added to 50 mL of 0.0700 M NaIO3. Determine the ff: a. Initial…

A: Given 75.0-mL sample of 0.003 M AgNO3 is added to 50 mL of 0.0700 M NaIO3  We have to find Initial…

Q: (vi) Determine whether a precipitate of AgCI(s) will form on mixing 50.0 mL of 1.0 x 10-4 mol L-1…

A: Please Find the attached images for the answer

Q: A solution containing lead (II) nitrate is mixed with one containing sodium bromide to form a…

A:

Q: 27. For PbCl2 (Ksp = 2.4 x 10-), will a precipitate of PbCl, form when 0.10 L of 3.0 x 10 M Pb(NOa)a…

A: Given that, 0.10 L of 3.0×10-2 M Pb(NO3)2 is added to 400 ml of 9.0×10-2 M NaCl. Ksp of PbCl2 =…

Q: 3. A solution has [Pb2+] = 0.0012 M and [CI] = 0.010 M. Will PbCl2 precipitate form? Ksp for PbCl₂ =…

A:

Q: What is the expression for the solubility product constant, Ksp, of calcium phosphate, Ca3(PO4)2…

A: Solubility product constant (Ksp); When a slightly soluble ionic compound is mixed with water,…

Q: Will a precipitate be observed if 0.10 mol Ag* and 0.001 mol SO4²- are added to make 1.0 L of…

A: Here we are required to find whether precipitation will occur or not

Q: 46. Given this solution at equilibrium: CaF2(s) = Ca2+(aq) + 2F-(aq)What is the solubility products…

A: Salts which are partially soluble in water attain equilibrium between dissolved forms and…

Q: Will a precipitate form when 20.0 mL of 1.8x10-3 M Pb(NO3)2 is added to 30.0 mL of 5.0x10-4 M…

A: Given Data :

Q: After mixing an execess PbCl2 with a fixed amount of water, it is found that the equilibrium…

A: First, the Ksp expression for given compound is determined.

Q: Will a precipitate form when 150 mL of 0.10 M Pb(NO3)2 are combined with 100 mL of 0.20 M NaCl? Ksp…

A: We can decide whether a precipitate will form or not on the bases of the Q and Ksp values. Qsp…

Q: A solution contains 0.0500 M Ca²+ and 0.0300 M Agt. Can 99% of Ca²+ be precipitated by sulfate…

A:

Q: Will a precipitate form when 400.0 mL of 1.2 x 10-3 M MgCl2 are added to 300.0 mL of 1.2 x 103 M…

A: After mixing, total volume of Solution is 400+300 = 700 mL MgCl2 and NaF are strong electrolytes,…

Q: 16. Equal volumes of 0.020 M Ag+ solution and 2.0 M NH3 solution are mixed. Kf for [Ag(NH3)2]+ is…

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

Q: At a certain temperature, 0.35 g of BaF2 (Molar mass = 175) dissolves in pure water to form 1L of…

A: Given : Mass of BaF2 in saturated solution = 0.35 g Volume of solution = 1 L And molar mass of BaF2…

Q: 31. For PbCl, (Ksp = 2.4 x 10-4), will a precipitate of PbCl, form when 0.10 L of 3.0 x 10-2M…

A: We have to choose whether ppt will be formed or not.

Q: Ksp

A:

Q: For PbCl2, Ksp 1.7 x 105. What will occur if 250 mL of 0.10 M %3D Pb(NO3)2 is mixed with 250 mL of…

A:

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.