MgNH4PO4•6H2O has the solubility of 0.023g/100ml. There is a precipitate of 0.7193g and a student washes it down with 50.0mL of water. How of the precipitate is left?

Q: b. CH3CH2OH + NaOH --> CH3CH2O - + NaOH2 +       c. CH3COOH + NaOH --> CH3COONa + H2O       d.…

A: We have to find out correct reaction between acetic acid and sodium hydroxide solution

Q: Calculate the solubility of Mercury (II) iodide (HgI2)(HgI2) when a 3.0 M solution of NaI is added,…

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Q: A saturated solution of magnesium hydroxide is prepared and the excess solid magneisum hydorixed is…

A: Solution :        Titration is used to find out the concentration of an unknown solution(titrand or…

Q: A 750 mL solution contains o.350 M K2Cro4, and a.350 M Na2SO4. A concentrated Ba(NO3)2 is slowly…

A: Ksp : At normal temperature, if the solubility of a salt is 0.1mol / Lit then that salt is called…

Q: The molar solubility of mercury (II) sulfide is below. What is the Ksp ? Molar solubility = 2.9 x…

A: given data from question -  molar solubility = 2.9 x 10-25 g/L Ksp = ?

Q: Calculate the molar solubility of Ca(IO3)2 in each solution below. The Ksp of calcium iodate is 7.1…

A: The solubility reaction of Ca(IO3)2 is  => Ca(IO3)2 (s) -------> Ca2+ (aq) + 2 IO3- (aq) The…

Q: The solubility (So) of Drug x free acid in water is 0.006M.The total concentration of Drug x (free…

A: Given that -  Concentration of free acid in drug = 0.006M  Concentration of free acid + salt in drug…

Q: 20.0g of NaOH(molar mass = 40.0g/mol)was mixed with 40.0g of AgNO3(molar mass =170.0g/mol)and the…

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Q: Calculate the solubility of FeCO3 (a) in pure water and (b) in a solution in which [Na2CO3] = 0.256…

A:

Q: 100mL of 0.200 M AgNo3  is mixed with 100mL of 0.100M Na2S04. How many grams of Ag2SO4 will…

A: To calculate the grams of Ag2SO4 precipitates , we would first write a balanced chemical equation.…

Q: 20.00 mL of 1.100 x 104 mol/L Pb(NO3)2 is mixed with 80.00 mL of a 4.450 x 10-2 mol/L Cal2. The Ksp…

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Q: Will a precipitate form when 75.0 ml of 0.020 M BaCl2 and 125 ml of 0.040 M Na2SO4 are mixed? (Ksp…

A: Given: The molarity of BaCl2 solution is 0.020 M. The volume of BaCl2 solution is 75.0 mL. The…

Q: 9. A flask containing 0.10 M NaCl (aq) and 0.010 M K₂CrO4 (aq) has some solid AgNO, added to it. Ksp…

A: #9: 1 mol NaCl is completely dissociated to give 1 mol Cl-(aq). Hence [Cl-(aq)] = [NaCl] = 0.10 M  1…

Q: use solubility to answer this   Calculate whether or not precipitate will be formed in each case…

A: Calculate whether or not precipitate will be formed in each case.,

Q: A solution contains 0.25 M Ni(NO3)2 and 0.25 M Cu(NO3)2. A. 1.Can the metal ions be separated by…

A: Given that, Ksp (CuCO3) = 1.4 x10-10Ksp (NiCO3) = 1.42 x10-7

Q: If 125 mL of a solution containing 0.0400 M of Pb(NO3)2(aq) is mixed with 75.0 mL of a solution…

A: We have to find whether there will be precipitate formation of PbCl2 or not.

Q: Calcium hydroxide has a solubility product constant of Ksp = 4. 68 × 10–6 Calculate the solubility…

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Q: Lead (II) Bromide is a slightly soluble solute in water. The following equation represents the…

A: The solubility, s, of the PbBr2 is calculated as shown below.…

Q: What is the molar solubility of AgCl (Ksp = 1.8 × 10−10)?   7.31 × 10−5 M   5.13 × 10−6 M   3.84…

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Q: The solubility of a certain salt A2D in a 0.05M solution of A(NO3) is 0.006 M. 1. Calculate the…

A: Le the initial solubility be denoted by 's': A2D will dissociate as: A2D→2A++D2-             2s…

Q: A solution is made by dissolving 0.1283 g of the acid form of the buffer TRIS (molecular mass =…

A: According to the mole concept, in terms of mass, the amount of substance in moles is equal to the…

Q: What can be said about the solution formed by adding 150.0 mL of 0.150 M CaCl2 with 100.0 mL of…

A: The chemical reaction of the CaCrO4 - Given, 150.0 mL of 0.150 M CaCl2  100.0 mL of 0.035 M H2CrO4…

Q: A 1500 mL solution contains 0.350 M K2CrO4 and 0.350 M Na2SO4. A concentrated Ba(NO3)2 is slowly…

A: The question is based on the concept of selective precipitation. we have a solution of sulphate and…

Q: If 50.0 g of barium arsenate (Ksp = 1.1 x 10-13) are placed in enough water to generate 500.0 mL of…

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Q: The first step in the preparation of magnesium metal is the precipitation of Mg(OH)2 from sea water…

A: Solubility product constant Kspis an equilibrium constant that is defined as the product of the…

Q: In which ONE of the following aqueous solutions is solid silver sulfate least soluble before a…

A:

Q: True or False

A: (1) Precipitimetry involves the use of Silver chloride as the titrant. Hence the other of this…

Q: Acetic acid (molecular weight = 60.05 g/mol) and sodium acetate (molecular weight = 82.03 g/mol) can…

A: Initial number of moles of NaOH, acetic acid and sodium acetate is determined as follows, 1 mL =…

Q: 100mL of 0.200 M AgNo3  is mixed with 100mL of 0.100M Na2S04. How many grams of Ag2SO4 will…

A: Volume of AgNO3 = 100 mL = 0.1L Molarity of AgNO3 = 0.200 M Volume of Na2SO4 = 100 mL Molarity of…

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: When a 100.0-mL portion of a solution containing 0.500 g of AGNO3 is mixed with 100.0 mL of a…

A: Given,  Volume of AgNO3 = 100.0 mL  Mass of AgNO3 = 0.500 g  Volume of K2CrO4 = 100.0 mL  Mass of…

Q: The Ksp for silver chromate ( Ag, CrO4) is 9.0 x 10 2. Calculate the solubility of silver chromate…

A: (a)

Q: Does a precipitate form for 100.0 mL of 0.002 M Na2CO3 are added to 100.0 mL of 0.002 M MgCl2. The…

A: Introduction: The product of the concentration of ions in a solution, which raised to the same power…

Q: If 50.0 g of silver phosphate (Ksp = 1.8 x 10-18) are placed in enough water to generate 500.0 mL of…

A:

Q: For the sparingly soluble salt, Ag3PO4 , calculate:   The molar solubility and the solubility in…

A: The solubility gets evaluated in mol/L is stated as "molar solubility". When any common ion is…

Q: The Ksp for Q, a slightly soluble ionic compound composed of M22+ and X- ions, is 4.5x10-29. The…

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Q: a) Theoretically, what would be the solubility product (Ksp) of an ionic compound having the general…

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Q: The Ksp of PbBr2 is 6.60× 10–6. What is the molar solubility of PbBr2 in 0.500 M KBr solution? What…

A: The solubility product (Ksp) expression for any compound is the mathematical product of the molar…

Q: 194. mL of 0.00104 M NaI (aq) is combined with 720. mL of 0.00499 M Pb(NO3)2 (aq). Determine if a…

A: Moles of NaI = (194*0.00104)/1000 = 0.000202  Moles of Pb(NO3)2 = (720*0.00499)/1000 = 0.00359…

Q: How quantity Qsp and Ksp can be used in predicting precipitate formation?

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Q: hat is 0.10M in AgNO3 and 0.075M in NaCl. What will happen once these solutions are mixed?…

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Q: If 25 mL of 2.00 × 10−2 mol/L sodium hydroxide is added to 80 mL of 3.2 × 10−2 mol/L magnesium…

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Q: At a certain temperature, the solubility product constant* of copper (II) iodate, Cu(IO3)2, is…

A: Since you have posted multiple questions, we are entitled to answer the first only.

Q: Copper(I) ions in aqueous solution react with NH, (aq) according to Cu*(aq) + 2 NH, (aq) → Cu(NH,);…

A:

Q: A solution contains 0.17 mol of KBr and 1.7 ✕ 10−5 mol of KCl per liter. CuNO3 is gradually added to…

A: Let us first write the equilibrium equation of the salt solution.  CuCl⇋Cu+ + Cl- The Ksp value for…

Q: 591. mL of 0.00499 M Nal (aq) is combined with 419. mL of 0.00325 M Pb(NO3)2 (aq). Determine if a…

A: Given, the Ksp of PbI2 = 1.40×10-8 We have to find whether a precipitate will form or not when 591…

Q: A sample solution contains two unknown ions. A student did a series of tests on the solution, in the…

A:

Q: Acetic acid (molecular weight = 60.05 g/mol) and sodium acetate (molecular weight = 82.03 g/mol) can…

A: Initial number of moles of NaOH, acetic acid and sodium acetate is determined as follows, 1 mL =…

Q: Potassium hydroxide is used to precipitate each of the cations from their respective solution.…

A:

Q: solution is 0.010 M in both KCl and NaBr. A lead sulfate solution is added dropwise until [Pb2+]…

A: The given information is: Concentration of KCl = 0.010 M Concentration of KBr = 0.010 M Lead sulfate…

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.