Calculate the equilibrium concentration of Cu2+ in a solution initially with 0.050 M Cu2+ and 1.00 M NH3.

Q: Write the mass-balance expressions for a solution that is a. 0.15 M in HF. 0.15 M HF F b. 0.16 M in…

A: When a chemical reaction occur mass of substance is conserved that is sum of masses of reactant is…

Q: Calculate the solubility of Mn(OH)2 in grams per literwhen buffered at pH (a) 7.0, (b) 9.5, (c)…

A:

Q: Calculate the molar solubility of Ni(OH)2 when buffered at pH 8.0.

A: Given:   The pH value of Ni(OH)2 is 8.0. The value of Ksp is not given. Thus, so it is taken from…

Q: 3) What is the solubility of AgCl if the Kp is 1.6 x 10 -10?

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

Q: Calculate the molar solubility of AgBr in 0.035 M NaBr (ksp = 5 x 10-13).

A: First the Ksp equation is noted.

Q: A buffer solution with a pH of 4.04 is prepared with the same volumes of 0.80 M HC2H;O2 and M…

A:

Q: Calculate the solubility of CaC2O4 in a solution containing 0.001 molarity H+

A: Solubility indicates the maximum amount of a substance that can be dissolved in a solvent at a given…

Q: The solubility products of Fe(OH)3 and Ni(OH)2 are about 10-36 and 6 × 10-18, respectively. Find the…

A: The minimum concentration of hydroxide to precipitate 0.1% of Fe3+ ion as Fe(OH)3 is calculated as…

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: Calculate the amounts of solids Na2HPO4 and NaH2PO4 needed to prepare 0.40 M, 1.5L of phosphate…

A:

Q: A buffer solution is made that is 0.384 M in HNO2 and 0.384 M in NaNO2 . (1) If Ka for HNO2 is…

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid

Q: Determine the pH of a buffer solution containing 0.150 M of NH3 and 1.2OM of NH&CI. K of NH3 = 1.8 x…

A: Buffer :-  A solution which resists the change in its pH value when small amount of strong acid or…

Q: Which salt can increase the solubility of Ag2SO4? O NazSO4 O silver acetate O AgNO3 NANO3

A: The maximum amount of salt which can be dissolved in the solution in such a way that after a certain…

Q: If 175 mL of a 0.0208 M AgNO3 solution is added to a 250 mL 0.0380 M K2CrO4, will Ag+ precipitiate…

A: Dissociation of Ag2CrO4 is given. Ksp value for the given reaction is taken as 1.1×10-12.

Q: In an experiment on evaluation of antacid containing magnesium carbonate, a tablet weighing 2.50 g…

A: Given, mass of tablet = 2.50 g            molarity of HCl = 1.00 M            volume of HCl = 5.00…

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: 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: A buffer solution is made that is 0.333 M in HNO2   and 0.333 M in NaNO2. If Ka for HNO2 is 4.50 x…

A: Since the solution is having weak monoprotic acid HNO2 and its conjugate base NaNO2  hence the…

Q: Calculate the molar solubility of CdCO3 in a buffer solution containing 0.115 M Na2CO3 and 0.120 M…

A:

Q: Calculate the molar solubility of Al(OH)3 in a buffer solution with 0.100 M NH3 and 0.400 M NH4+.

A: Base dissociation constant Kb for ammonia is 1.8×10-5. NH3aq+H2Ol⇔NH4++OH- Kb=NH4+OH-NH3

Q: A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in LiF. Calculate the pH of the solution after…

A:

Q: e the solubility-product constant of AgCl. AG¡X for the dissolution of AgBr(s). e the…

A: The question is based on the concept of chemical thermodynamics. we have to calculate solubility…

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: Calculate the mass of Cd(OH)2 that will dissolve in a buffer made by combining 400.0 mL of 8.0 M NH3…

A: Henderson hasselbalch equation: pOH=pKb+log[conjugate acid][weak base]

Q: From the value of Kf, calculate the concentration of Ni2+ (aq) and Ni(NH3)62+ that are present at…

A: Given: Mass of NiCl2=1.25 g Volume of NH3(aq)=100 mL Concentration of NH3(aq)=0.20 M

Q: Calculate the concentration of ammonium ion that is required to prevent the precipitation of Mg(OH)2…

A: Solubility product constant Ksp: It basically shows the strength of solute to dissolve in aqueous…

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: 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…

A:

Q: Determine the molar solubility of AgCl in a 1.0 M solution of NH3. Kp of AgCI - 1.ó x 10 10 K of…

A: Given, Concentration of NH3 = 1M Ksp of AgCl is =1.6× 10^ -10. Kf of Ag(NH3)2 + = 1.5 × 10^7. We…

Q: What will be the effect of adding the following solutions on the solubility of the slightly soluble…

A: a). When K2CrO4 is added to the solution of a slightly soluble ionic compound (BaCrO4 ) then the…

Q: calculate the molar solubility of AgBr in 0.10 M NaBr solution.

A: Solubility is defined as the amount of solute dissolved in the particular amount of solvent at a…

Q: In which solution would the molar solubility of AgCI be lowest? (A) pure water (B) 0.10 M CaCl2 (C)…

A: Correct choice is (B)  This problem is based on the common ion effect of solubility.  We know that…

Q: Calculate the molar solubility of Ni(OH)2 when buffered at pH 12.0

A: To calculate the molar solubility of Ni(OH)2 when pH 12.0. The solubility product of Ni(OH)2 is…

Q: Calculate the molar solubility of Ni(OH)2 when buffered at pH 14.0

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

Q: Calculate the solubility of Mn(OH), in grams per liter when buffered at pH = 9.7.

A:

Q: At pH 10.0, only 0.019 g of MgCl2 will dissolve per 1 L of solution. What is the Ksp of magnesium…

A: The pH is given as 10.0 Therefore pOH = 14-pH = 14-10.0 =4.0 Then the pOH = -log[OH-] So, [OH-] =…

Q: Calculate the molar solubility of Ca(IO₃)₂ in (a) 0.060 M Ca(NO₃)₂ and (b) 0.060 M NaIO₃

A: Introduction: Solubility: It is defined as the maximum amount of solute that can be dissolved in the…

Q: Calculate the pH at the equivalence point for the titration of 0.110 M methylamine (CH,NH, ) with…

A: We need to find pH at equivalence point.

Q: What mass of AgBr will dissolve in 500.0 mL of 1.35 M NH₃? Ksp for AgBr is 5.0 × 10⁻¹³. For the…

A: The two equations as per the question along with their rate constants are given below:- Ag+(aq)    +…

Q: Calculate the pH of the buffer solution produced from the addition of 0.030 L of 0.150 M KOH to…

A: For a buffer pH = pKa + log C2/c1

Q: Calculate the pH of a buffer that is 0.225 M HC2H3O2 and 0.162 M KC2H3O2. The Ka for HC2H302 is 1.8…

A: Given: Concentration of HC2H3O2 = 0.225 M Concentration of KC2H3O2 = 0.162 M Ka for HC2H3O2 =…

Q: calculate the molar solubility of AgBr in 3.0 * 10-2 M AgNO3 solution.

A: Given that: concentration of AgNO3 = 3.0×10-2 M To find: The molar solubility of AgBr? Silver…

Q: Calculate the solubility of Ba(103)2 in a solution prepared by mixing 200 ml of 0.0100M Ba(NO3)2…

A:

Q: Determine the molar solubility of AgBr in a solution containing 0.150 M NaBr. K sp (AgBr) = 7.7 × 10…

A: Given, Ksp of AgBr = 7.7×10-13 Concentration of NaBr = 0.150 M The reaction of complete dissociation…

Q: The solubility product constant of Mg(OH) is 1.8 x 10-11 at 25°C. Calculate the pH of a 2saturated…

A: The solubility product constant of Mg(OH)2 is 1.8 x 10-11 at 25°C. Calculate the pH of a saturated…

Q: What concentration ratio of NH3 to NH4Cl is necessary to get a buffer solution with a pOH of 5.3? Kb…

A:

Q: What concentration of SO 3 ^ 2- is in equilibrium with Ag2SO3(s) and 1.60 x 10^-3 M Ag^+?

A: [Ag+] = 1.60 x 10-3 M  Ksp of Ag2SO3 = 1.5×10-14

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.