What is the minimum concentration of SO2−4 required to precipitate BaSO4 in a solution containing 1.0×10−4 mol Ba2+? (Kspfor BaSO4 is 4×10−10)

Q: Calcium oxalate, CaCO4, is very insoluble in water. What mass of sodium oxalate,Na2C2O4, is required…

A: Given: Volume of CaCl2 = 37.5 ml Molarity of CaCl2 = 0.104M

Q: Suppose you have a solution that might contain any or allof the following cations: Ni2+, Ag+, Sr2+,…

A: Among the ions, Ag and Sr are the only two that will react with these ions to form precipiate.

Q: It requires 7.65 mL of 0.100 HCl solution to neutralize (titrate) 25.00 mL of Ba(OH)2 solution. What…

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Q: 2. A buffer solution of volume 0.500 L contains 1.68 g NH3 and 4.05 g (NH);SOu. a) What is the pH of…

A: “Since you have asked multiple questions, we will solve the first question [Q2] for you. If you want…

Q: Potassium hydrogen phthalate (KHP) is often used as a primary standard in acid–base titrations. If…

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Q: Is BaF2 soluble in water, and if so, what ion is produced

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Q: What is the nitrate ion concentration in the final solution when 50mL of 0.5M NaNO3 is mixed with…

A: The concentration of solute in the given solution is given in the term of molarity.

Q: Solid barium chloride is slowly added to 150 mL of a potassium sulfite solution until the…

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Q: The term buffer capacity is difficult to define exactly because it is defined differently with each…

A: We can find the Concentration of the Compound in solutions by using Molarity, Normality . If the…

Q: 200. mL of 0.50 M NaCl and 800. mL of 0.100 M AgNO3 are mixed together. Calculate the mass of the…

A: Double displacement reactions are basically the reactions in which exchange of various ions takes…

Q: If a 0.2501 g sample of sodium bicarbonate (96.5% NaHCO3) is titrated with 0.1165 N sulfuric acid,…

A: Given data : g NaHCO3 = 0.2501 × (96.5/100) g N H2SO4= 0.1165 meq/mL Molar mass of NaHCO3 = 84 g/mol

Q: How many grams of nickel (II) phosphate (366.02 g/mol) will precipitate if excess sodium phosphate…

A: The balanced equation for the reaction is given below.

Q: What is the concentration of F— ions when 266.640 mg of MgF2 (62.3018 g/mol) completely dissociates…

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Q: 3a. (2)A student prepared a 0.0750 M NaOH solution for a titration experiment. If it took 25.52 ml…

A: Here in a titration 25.52 ml of NaOH aqueous solution is consumed at equivalent point when titrated…

Q: 0.0500 M HF (Ka= 7.20 x 10–4)  determine the equilibrium molar concentration of H3O+ and…

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Q: If a solution contains 0.0020 mol of CrO4 2− per liter, what concentration of Ag+ ion must be…

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Q: hat is the formula of the precipitate that forms when aqueous Fe(NO3)3 and aqueous NaCO3 are mixed?

A: Double displacement reaction-in reaction positive and negative ions of two ionic compounds displaces…

Q: You have a solution of 1M BaCl2 and another of 1M Hg2(NO3)2. If you poured them together, what…

A: 1. In double displacement reaction,  cation of one species easily replaces cation of another species…

Q: Which of the following is the least soluble in water? Lithium hydroxide Lithium sulfide Silver…

A: Some of the ionic compounds dissociate completely in an aqueous solution (strong electrolyte) and…

Q: NaCl is purified by adding HCl to a saturated solution of NaCl (317 g/L). When 28.5 mL of 8.65 MHCl…

A: Calculation of the molarity of the initial NaCl solution: M=317 g/L58.44 g/mol=5.424 mol/L…

Q: If it required 23.9 mL of 0.0150 M Ca(OH)2 to neutralize 25.0 mL of HNO3 , what was the initial…

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Q: 5 A chemistry graduate student is given 450. mL of a 0.10M ammonia (NH3) solution. Ammonia is a weak…

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Q: You are titrating 10.00 mL 0.100 M H3PO4 with 0.100 M NaOH. At the point where you have added…

A: H3PO4 (aq)  + Na+(aq) + OH- (aq)  →   Na+(aq) + H2PO4-(aq) + H2O…

Q: If 600 mL of some Pb(NO3)2 solution is mixed with 200 mL of 2.80 x 10−2 M NaCl solution, what is the…

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Q: A student performs a titration of 53.0 mL of a phosphoric acid (H₂PO₂) solution of unknown…

A: 53.0 mL of phosphoric acid H3PO4 solution is titrated with 1.25 M of 26.2 mL NaOH solution to…

Q: A 50.0 mL solution of Ca(OH)2 with an unknown concentration was titrated with 0.340 M HNO3. To reach…

A: Neutralization :- The reaction of an acid with a base to form salt and water is known as…

Q: What [Ag*] is needed to just begin precipitating Ag2SO4 (s) from a .0073 M SO42 (aq) solution? O 4.7…

A: The solubility product, Ksp is the product of dissolved ion concentration raised to the power of…

Q: Potassium hydrogen phthalate (KHP) is often used as a primary standard in acid–base titrations. If…

A: Given information: Volume of NaOH = 19.45 mL Gram of KHP = 0.397 g

Q: 1)Write a balanced chemical equation for the reaction of ammonia and hydrochloric acid and a…

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Q: Will the following reaction yields a precipitate? yes or no   Pb(NO3)2(aq)  +  NaC2H3O2(aq) ->

A: The precipitation reactions are the reactions involving the formation of insoluble solid product,…

Q: 45.21 mL of NaOH is used to reach the endpoint in titrating 0.8001 g KHP (204.22 g/mol). How much of…

A: The nfactor for NaOH is 1, for KHP is 1 and for H2SO4 is 2.

Q: 4. The concentration of a NaOH solution is determine by using the solution to titrate a sample of…

A: The objective of the question is to calculate the concentration of a sodium hydroxide (NaOH)…

Q: The solubility constant of lead (II) hydroxide [Pb(OH)2] is 1.2 x 10-15.  If 100.0 g of this…

A: The molar solubility (s) of [Pb(OH)2] is calculated as shown below. On substitution, the molar…

Q: A solution contains 1.44×102 M sodium carbonate and 1.08×102 M ammonium sulfide. Solid manganese(II)…

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

Q: Will a precipitate of SrF2 form if you mix 25 mL of 7.1 x 10^-2 M Sr(NO3)2 (aq) with 85 mL of 3.2 x…

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Q: With the given plot, if a 0.1000 M NaOH solution was used to fully precipitate all the Zn2+ in the…

A: Answer: In this question we have to convert moles of NaOH into moles of Zn2+ ion to find out the…

Q: If 550 mL of some Pb(NO3)2 solution is mixed with 100 mL of 7.50 x 10−2 M NaCl solution, what is the…

A: Given information: Volume of Pb(NO3)2 solution is 550 mL Volume of NaCl solution is 100 mL…

Q: A Fajans titration of a 0.7908-g sample required 45.32 mL of 0.1046 M AgNO3. Express the results of…

A: Step : 1            Express the results of this analysis in terms of the percentage of BaCl2·H2O.

Q: in NH3 and 0.5 M in HCl is (Kb for NH3 = 1.8 x 10¯5):   (A) a solution with a pH less than 7 that…

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Q: 7. The separate samples of nitric and acetic acids are both titrated with a 0.100 M solution of…

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Q: Solid ammonium carbonate is slowly added to 150 mL of a 0.0645 M magnesium acetate solution. The…

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Q: To simulate the pH of blood, which is 7.4, an undergraduate researcher in a biology lab produced a…

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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.