What is the solubility of AgCN(s) (Ksp = 2.2 × 10⁻¹⁶) in a solution containing 0.55 M H⁺? (Ka for HCN is 6.2 × 10⁻¹⁰.)

Q: A 50.0 mL sample of 0.100 M NH3 is titrated with 0.100 M HBr. What is the most likely pH of the…

A: The pH of the solution is the power of protons in the solution. While pOH is related to the basicity…

Q: Under what circumstances, if any, does a sample of solid AgCl completely dissolve in pure water?

A: The number of moles of a solute that is dissolved per litre of solution is termed as Molar…

Q: Calculate the molar solubility of Cr(OH)3 in 0.50M NaOH; Kf for [Cr(OH)4]- is 8 x 10^29.

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Q: What is the pH of a buffer made from 0.220 mol of HCNO (Ka = 3.5 × 10 4) and 0.410 mol of NaCNO in…

A: Henderson's Equation:- This equation gives the pH of a buffer solution.  The number of moles of salt…

Q: A buffer is composed of 0.200 M (CH3)2NH (Kb = 5.9 x 10-4) and O.250 M (CH3)2NH2NO3 . What is the pH…

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Q: B. In an acid-base titration, a solution of 50.0 ml of hydrochloric acid is completely neutralized…

A: Given:  The volume of HCl = 50 mL The volume of KOH = 25 mL The concentration of KOH = 0.80 M

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 barium fluoride in: (a.) pure water (b.)0.10 M Ba(NO3)2 (c.)0.15…

A: Here We have to calculate the molar Solubility of barium fluoride in different solvents given…

Q: Consider a buffer made by adding 132.8 g of NaC₇H₅O₂ to 300.0 mL of 1.09 M HC₇H₅O₂ (Ka = 6.3 x 10⁻⁵)…

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Q: 13. Which is the solubility in moles per liter of Ca(OH)2 in 0.5 M NAOH solution?

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Q: Consider a buffer made by adding 48.3 g of (CH3)2NH2I to 250.0 mL of 1.42 M (CH:)2NH (Kb = 5.4 x…

A: Answer:- This question is answered by using the simple concept of calculation of pH of a buffer…

Q: . What is the pH of a buffer prepared by adding 0.405 mol of the weak acid HA to 0.507 mol of NaA in…

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Q: Describe how the presence of a common ion reduces the solubility of an ioniccompound.

A: The presence of a common ion reduces the solubility of an ionic compound has to be described below.

Q: in terms of Ksp What is the molar solubility, s, of Ba,(PO)2

A: Ba3(PO4)2→sparingly soluble salt ( partially dissociate into ions)Ba3(PO4)2⇌3Ba2++2PO43- Molar…

Q: What is the molar solubility (in M) of PbCl2 in a 0.15 M solution of HCI? The Ksp of PbCl2 is 1.6 x…

A: Introduction The solubility product is equivalent to product of the corresponding ions of any…

Q: A buffer consists of 0.21 M H3PO4 and 0.38 M NaH2PO4. Given that the K values for H3PO4 are, Ka1 =…

A: Given that, a buffer is made by 0.21 M of H3PO4 and 0.38 M of NaH2PO4. The dissociation constant…

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: Calculate the molar solubility of solid Ca(OH)2 (Ksp = 6.5 x 10-6) in each of the following.  Water…

A: To calculate the molar solubility of solid Ca(OH)2 in each of the following. Water A 0.125 M…

Q: When solid silver chloride is added to 100. mL of H2O, 1.9 x 10–4 grams dissolves. What is the Ksp…

A: Solubility product

Q: Calculate the molar solubility of CaF2 at 25 °C in a solution that is 0.010 M in Ca(NO3)2

A: CaF2 dissociates as                     CaF2 (s)  →  Ca+  +  2F- Initial…

Q: Consider a buffer made by adding 132.8 g of NaC,H;O2 to 300.0 mL of 1.31 M HC,H;O2 (Ka = 6.3 x 105)…

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Q: What is the pH of a buffer that contains 0.15 M CH3COOH and 0.10 M NaCH3COO (K, = 1.8 x 10$)?

A: Given : Concentration of weak acid CH3COOH = 0.15 M And concentration of conjugate base salt of weak…

Q: What are the concentrations of Ag+, CN–, and Ag(CN)2 − in a saturated solution of AgCN?

A: In the 1.0 L of a saturated AgCN solution, the concentration of Ag+ and CN- is;…

Q: Calculate the solubility in g/100 mL of the AgI in 0.10 M NH3 . The NH3 concentration is that of…

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Q: Tris(hydroxymethyl)aminomethane is a common base used to prepare buffers in biochemistry.  Its Kb is…

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Q: Consider a buffer made by adding 132.8 g of NaC₇H₅O₂ to 300.0 mL of 1.09 M HC₇H₅O₂ (Ka = 6.3 x 10⁻⁵)…

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Q: 1. What is the pH of a buffer that contains 0.15 M CH,COOH and 0.10 M NACH,COO (K, = 1.8 x 10 )?

A: 1) Given, Concentration of CH3COOH solution = 0.15 M [CH3COOH] = 0.15 M Concentration of NaCH3COO…

Q: ) Lead(II) hydroxide, Pb(OH)2 consists of lead(II) ion and hydroxide ion. Given that Kyp value of…

A: Solubility product is an equilibrium constant which is determined by multiplying the concentration…

Q: Ksp for PbSO4 is 1.3 x 10–8 . Pb ions form a complex ion [PbI4] 2− in the presence of KI, which has…

A: The chemical equation for the dissociation of PbSO4(s) is: PbSO4(s) ⇌ Pb2+(aq) + SO42-(aq) ; Ksp =…

Q: 4.) A solution contains 7.84 x 10 8 M of copper ion (Cu2*) and has a pH of 9.118. Does copper(II)…

A: Given that:  [Cu2+] = 7.84×10-8M pH = 9.118  Ksp of Cu(OH)2 = 1.10×10-15 Using: pH + pOH = 14 pOH =…

Q: Calculate the molar solubility of solid Ca(OH)2 (Ksp = 6.5 x 10^-6) in 0.125 M solution of Ba(OH)2…

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Q: Calculate the solubility of LaF3 in grams per liter in 0.050 M LaCl3 solution.

A: Given: LaCl3 solution= 0.050M Calculate solubility of LaF3  =?   Molar mass of LaF3 = 195.90 g/mol…

Q: Consider a buffer made by adding 52.3 g of (CH3),NH2I to 250.0mL of 1.42 M (CH3)¿NH (Kb = 5.4 x…

A: The concentration or Molarity of salt is calculated by - M = w×1000/m×V Here, M = Molarity of Salt,…

Q: a. What is the pH of an aqueous solution of 100.0 mL with 1.00 mmol Ca(OH)2 (74.1 mg) dissolved in…

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Q: Tris(hydroxymethyl)aminomethane is a common base used to prepare buffers in biochemistry. Its Kb is…

A: To calculate pH of a basic buffer , we would first calculate its pOH using Henderson-Hassalbalch…

Q: Describe the effect of pH on the solubility of Fe(OH)3

A: A reaction is said to be in equilibrium if the rate of the forward reaction is equal to the rate of…

Q: Calcium hydroxide (Ca(OH)a) is a strong base. Its solubility is about 0.74 g/L at 25°C. 1. For a…

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Q: what is the ph of a buffer that consists of 0.86 m HBrO (ka= 2.29 x 10-9) and 0.41 M KBr

A: The pH of a buffer solution can be determined using Handerson Hasselbach equation that suggests the…

Q: If the molar solubility of silver bromide (AgBr) is 5.7x10-13, what is its Ksp?

A: The solubility is taken as ‘s’. The expression for Ksp calculation is as shown below:…

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: 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 K for PbBr2 if its molar solubility is 2.14 x 10-2 M at 25°C.

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

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: What is the pH of a buffer made from 0.220 mol of HCNO (Ka = 3.5 × 10⁻⁴) and 0.410 mol of NaCNO in…

A: Henderson's equation for the calculation of buffer solution consisting of a weak acid and salt of…

Q: A general chemistry student performs a titration with 28.4 mL of 0.294 M weak acid solution with a…

A: Introduction The details and data about the H+ ions (hydrogen ions) are derived by deriving any…

Q: Consider a buffer made by adding 42.3 g of (CH3)2NH2I to 250.0 mL of 1.42 M (CH:)»NH (Kb = 5.4 x 10…

A: pH is a scale which is used to determine the acidity or basicity of a solution. pH = pKa + log…

Q: A certain weak acid, HA, with a K. value of 5.61 x 10-6, is titrated with NaOH.

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Q: The Ka of hyperchlorous acid, HClO is 3.50 X 10-8. How many grams of NaClO (molar mass = 74.5…

A: 1- First calculate the concentration of NaClO :  Using the Henderson equation,  pH = pKa +…

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.