Calculate the mass of potassium cyanide ion that must be added to 100 mL of solution to dissolve 2.0 × 10–2 mol of silver cyanide, AgCN.

Q: Complete the following solubility constant expression for SrCO 3.

A: SrCO3 ionises as : SrCO3 ----------> Sr2+ + CO32- Solubility product Ksp = [Sr2+][CO32-] Let the…

Q: Complete the following solubility constant expression for Fe(OH)2

A: Given -> Fe(OH)2

Q: The graph below shows the results obtained by titrating a different weak acid, H2Y, with the…

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Q: why does the volume of water added to dissolve the potassium hydrogen phthalate, KHP, not matter?

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Q: Briefly explain how one can increase the solubility of Ca3(PO4)2, a relatively insoluble compound?

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Q: Solid ammonium phosphate is slowly added to 150 ml of a 0.0595 M aluminum nitrate solution. The…

A: Ammonium Phosphate react with Aluminium Nitrate to form a solid precipitate of Aluminiun Phosphate.

Q: A buffer is made by dissolving 10.5 g of sodium dihydrogen phosphate, NaH2PO4 and 12.0 g disodium…

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Q: 1) Write the solubility constant expression for the following species: a) MnS b) AI(ОH)з с) Саз…

A: As per regulations only first question can be answered.

Q: At 25 degrees Celsius, what is the pH of a buffer that contains 0.100 M dimethylammonium chloride…

A: dimethyl amine has pKa = 3.27

Q: Define equivalence point, and describe the steps involved in determining it for weak acid-strong…

A: It is the point at which the amount of base added has completely neutralized the acid solution.At…

Q: In which case would the molar solubility of NİBR2 be the lowest? 0.10 M CaBr2 O 0.15 M HBr pure…

A: The solubility of salts decreases when we get common ions from other salts  Hence more the…

Q: Define the following terms: titration equivalence point buffer point molarity What instrument are…

A: 1. Titration  = It is a laboratory method of quantitative chemical analysis in which the solution of…

Q: A chemistry graduate student is given 250. mL of a 1.10 M trimethylamine ((CH;),N) s solution.…

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Q: A chemistry graduate student is given 300. mL of a 1.00M trimethylamine ((CH, N solution.…

A: The question is based on the concept of buffer solution.   A buffer is a solution which resist any…

Q: Calculate the molar solubility of calcium hydroxide in a solutionbuffered at each pH.a. pH = 4b. pH…

A: Molar solubility is defined as the number of moles of solute that can be dissolved in a solute…

Q: Lead (IV) hydroxide, Pb(OH)4 is a slightly soluble compound. 1. Write the dissolution equations for…

A: Solubility is defined as the amount of solute that dissolves in a solvent. For example: sugar…

Q: Describe how you can increase the buffering capacity of a 0.1 M acetate buffer

A: To give the method to increases the buffering capacity of a 0.1 M acetate buffer.

Q: Solid ammonium carbonate is slowly added to 175 mL of a 0.0606 M magnesium nitrate solution. The…

A: When ammonium carbonate is slowly added to magnesium nitrate solution, the products of the reaction…

Q: Consider an analyte solution of 50.0 mL of 0.050 M hydrochloric acid, HCl, titrated against 0.10 M…

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Q: Solid copper(II) acetate is slowly added to 75.0 mL of a 0.0646 M ammonium carbonate solution. The…

A: Copper (II) carbonate i.e CuCO3 salt is insoluble in water. And since the solution is having…

Q: Suppose we have a formula for the titration function P(x). What calculation would we want to do to…

A: Weak acids dissociate partially in an aqueous solution to furnish the hydrogen ions. The extent to…

Q: What is the molar solubility of Al(OH)3 in a solution containing 1.3 10-3 M NaOH?

A: Since the solution is having NaOH which is completely soluble in water. The complete dissociation…

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: Write the solubility product expression for copper (II) hydroxide, Cu(OH)2?

A: The solubility of a salt is the maximum amount that can be dissolved in a certain amount of water at…

Q: What are buffers in terms of acid-base equilibria, give an example, and can a buffer capacity be…

A: Buffer solution is a solution that is maintaining it's hydrogen ion concentration pH. With only…

Q: A chemistry graduate student is given 300. mL of a 1.80M acetic acid (HCH, CO,) solution. Acetic…

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Q: Write the net ionic equation in which the slightly soluble salt magnesium oxalate, MgC2O4, dissolves…

A: An equation which involves only those species which are involved in the reaction is referred to as a…

Q: Given lead (I1) hydraxide Pb (OH),what is the molar solubility? K" 1.2x10 iwhat is the pH of this…

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

Q: Calculate the pH of a buffer solution which contains the weak monoprotic acid, propanoic acid…

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Q: The Henderson-Hasselbalch equation relates the pH of a buffer to the relative concentrations of the…

A: Buffer solution is prepared, when an strong base is added into weak acid solution then resulting…

Q: Calculate the Potassium Hydrogen Phthalate (KHC8H4O4) titer of 0.125 M KOH.

A: Neutralization reaction: Equivalent amount of acid reacts with an equivalent amount of base This…

Q: What is the pH of a saturated solution of magnesium hydroxide (the active ingredient in the antacid…

A: Milk of magnesia which is a saturated solution of magnesium hydroxide has a pH of  about 10.0 (basic…

Q: A chemistry graduate student is given 250. mL of a 0.30M chloroacetic acid (HCH,CICO,) solution.…

A: We have to calculate the mass of salt added.

Q: If 4.5 moles of nitric acid falls into 8000 L of pure water, what will be the change of the pH of…

A: concentration = mole / litre concentration  = 4.5/8000L                         [ H+]= 0.5625 × 10-3…

Q: What mass (in grams) of potassium acetate, KC2H302, must be added to 145 ml of 0.010 M acetic acid…

A: Given  PH = 4.67  Ka  = 1.8 × 10-5 Molarity of acetic acid = 0.010 M Mass of potassium Acetate = ?

Q: Write the titration reaction of 100 mL of 0.100 M anilinium bromide (“aminobenzene . HBr”) +.100 M…

A: In analytical chemistry, titrations are carried out to determine the concentrations of unknown acids…

Q: A student pharmacist prepared a buffer solution by mixing 68 ml of 0.17 M ammonia and 42 mL of 0.12…

A: The working formula is  V1×S1 = V2×S2 V1 = initial volume V2 = final volume S1 = initial…

Q: Calculate the pH for each of the following cases in the titration of 60.0 mL of 0.250-M hydrobromic…

A: As per our guidelines, we are supposed to answer only one question with three sub parts. Kindly…

Q: What is selective precipitation? Under which conditions does selective precipitation occur?

A: What is selective precipitation? Under which conditions does selective precipitation occur?

Q: Calculate the cadmium ion concentration, [Cd2+], in a solution prepared by mixing 0.100 L of 0.0100…

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Q: Explain the role of a buffer, such as an antacid table or sodium bicarbonate, on the pH of a…

A: The antacids play an important role in controlling the pH of the body solution (like blood).…

Q: A chemistry graduate student is given 125. mL of a 1.30M dimethylamine ((CH,) NH) solution.…

A: Buffer solution:  It is a special type of mixture of a weak acid or a weak base and its conjugate…

Q: Write a general expression for the solubility constant of a compound with the general formula AmXn.

A: Solubility constant of a compound is equal to the product of the concentrations of ions raised to…

Q: How would the solid Pb(OH)2 (came from KOH) solubility be affected when hydrochloric acid is added?

A: Pb(OH)2(s) ---> Pb+2(aq) + 2OH-(aq)  Hcl(aq) ---> H+(aq) + Cl-(aq)

Q: Describe the Henderson Hasselbalch equation and explain its use in making buffers.

A: Buffer solutions are those solutions which resist in change of its pH for a  short range of change .…

Q: Define and explain the significance of the equivalence point of a titration. Identify the role of…

A: The equivalence point is a point of titration where the amount of added  titrant is enough just to…

Q: Calculate the molar solubility in units of moles per liter (Molarity) for the calcium (Ca^2+) and…

A: Given that:  Ksp of CaSO4 = 2.40×10-5 Ksp is solubility product constant which tells the solubility…

Q: A chemistry graduate student is given 300. mL of a 0.80 M methylamine (CH, NH,) solution.…

A: Given: Volume of solution = 300 mLMolarity of CH3NH2 = 0.80 MpH of solution = 10.92Kb of CH3NH2 =…

Q: Sketch the general appearance of the curve for the titration of a weak acid with a strong base.…

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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.