10.0 ml of HCl was added to 100.0 ml of a 0.2 M solution of NH4Cl (Ka=1.8x10-5). If the resulting equilibrium pH was 1.4, what was the concentration of the HCl solution?

Q: At 22 °C, an excess amount of a generic metal hydroxide, M(OH),, is mixed with pure water. The…

A: The balanced reaction is, M(OH)2 → M+2 + 2OH-Ksp=M2+OH-2   The pOH is, pOH = 14 - 10.38 = 3.62   So,…

Q: A common buffer solution can be prepared by using ammonia and ammonium salts. The base equilibrium…

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Q: CaF2 (5g) is placed in 1 L of O.1 M NaF and allowed to come to equilibrium. The Ksp (CaF2) = 5.3 x…

A: Solubility of a solid is the ability of it to dissolve in a solvent. The solubility of different…

Q: At 22 °C, an excess amount of a generic metal hydroxide, M(OH),, is mixed with pure water. The…

A: In order to find Ksp of the salt we first write down the given data: pH= 10.34. The given salt is…

Q: NH3 is a weak base (Kp = 1.8 × 10-5) and so the salt NH,Cl acts as a weak acid. What is the pH of a…

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Q: Which of the fellowing aqueous solutions are good buffer systems? O0.38 M hypochlorous acid + 0.25 M…

A:

Q: How many g of sodium formate should be added to 250 ml of 0.2 M hydrochloric acid solution to obtain…

A: Given,  Volume of HCl = 250 mL  Molarity of HCl = 0.2 M  pH = 4.3  Mass of sodium formate in g = ?

Q: 1.00 L of a buffer solution is prepared based on a weak acid, HA, with pKa = 4.536, where [HA] =…

A: A buffer is a solution which resist any change in pH on adding a small amount of acid or base . it…

Q: What is the equilibrium concentration of chloroacetic acid, HC₂H₂O₂Cl, in a solution prepared by…

A: Given: Moles of HC2H2O2Cl = 0.0271 mol Volume of water = 1.50 L Ka of HC2H2O2Cl = 1.4×10-3

Q: consisting

A: The neutralization reaction after the addition of strong base results into following changes-

Q: solution made by adding soilid NaClO to water resulted in a baasic equilibrim with a pH of 10.50.…

A: Given data set: Volume = 2 L pH = 10.50 Ka(HClO) = 3.0*10-7 Calculating the value of pOH using the…

Q: K = 1.4 x 10-3) and 0. %3D

A: Given data are as follows: Weak base = 0.260 M Conjugate acid =0.530 M Kb= 1.4*10-5

Q: The Ką of acid HA is 3.5 x 10 and the Kp of base B is 7.2 x 104. When 0.50-mol HA and 0.50-mol B are…

A: Answer: greater than 7

Q: What are the molar concentrations of acetic acid (CH,COOH) and sodium acetate (CH, COONA) in an…

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Q: 1) The equation below represents the equilibrium process of a saturated solution of Ca(OH)2 If the…

A: "Le Chatelier's principle" is mainly utilized for the prediction of effect of some various changes…

Q: Write the chemical reactions whose equilibrium constants are Kp and Ką for imidazole (C,H,N,) and…

A:

Q: A chemistry graduate student is given 450. mL of a 0.70M methylamine (CH3NH₂) solution. Methylamine…

A: The objective of the question is to calculate the mass of .

Q: At 22 °C, an excess amount of a generic metal hydroxide, M(OH),, is mixed with pure water. The…

A:

Q: The ionization constant (K») of aniline (CsHsNH2) is 2.35 x 10-5, If 7.285 grams of aniline is…

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

Q: CH,NH, is a weak base (Kp = 5.0 × 10-4), so the salt CH,NH,NO, acts as a weak acid. What is the pH…

A: Given, Kb for CH3NH2 = 5.0 × 10-4 We have to calculate the pH of a solution that is 0.0670 M in…

Q: 10.0 ml of HCl was added to 100.0 ml of a 0.2 M solution of NH4Cl (Ka=1.8x10-5). The resulting…

A: Given values  Volume of HCl= 10.0ml Volume of NH4Cl = 100ml Molarity of NH4Cl = 0.2M pH= 1.4

Q: Acetic acid and its conjugate base acetate can form an acid-base buffer.  The pKa of acetic acid is…

A: Given: Concentration of HNO3 = 10.0 M Concentration of acetic acid = 0.0100 M Concentration of…

Q: Determine the pH of a buffer solution that is a mixture containing 0.10M acetic acid and 0.050 M…

A:

Q: 1. 50.0 ml of 0.1 M NaOH is added to 100.0 ml of 0.2 M HCN (Ka=6.2x10-10). What is the pH of the…

A: Since you have posted multiple questions, we are entitled to answer the first only. 1) Given:…

Q: you mix 100. mL of 0.11 M HCl with 50.0 mL of 0.22 M NH3, what is the pH of the resulting solution?…

A: Volume of HCl=100.0mL Concentration of HCl=0.11M Volume of NH3=50.0mL Concentration of NH3=0.22M For…

Q: What change will be caused by addition of a small amount of Ba(OH)2 to a buffer solution containing…

A: Here, we have to find the change that will occur when a small amount of Ba(OH)2 is added to a buffer…

Q: Which of the following aqueous solutions are good buffer systems? O 0.38 M barium iodide + 0.27 M…

A: Buffer solution formed by combination of weak acid or base with salt of weak acid or base…

Q: The Solubility Product Constant for lead chromate is 1.8 × 10-¹4. If lead chromate is dissolved in…

A: The solubility product constant (Ksp) demonstrates the equilibrium between a solid and its…

Q: A student was required to prepare 250.0 mL of a cyanoacetic acid/sodium cyanoacetate buffer in which…

A: Given: Volume of buffer = 250.0 mL. Concentration of weak acid available = 0.51 M Concentration of…

Q: A buffer solution contains formic acid and a salt solution containing sodium formate. What is the pH…

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Q: A buffer solution contains 1.7 M acetic acid and 2.6 M sodium acetate. The Ka  of the acetic acid is…

A: Calculation of pKa of acetic acid: pKa=-log Ka=-log (1.8×10-5)=4.745

Q: 10.00 mL of 0.45 M NaOH is added to 9.00 mL of 1.00 M HCOOH. What is the molar concentration of…

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Q: A buffer is prepared by dissolving 0.80 mol of sodium dihydrogenphosphate, NaH2PO4, and 0.60 mol of…

A: Moles of sodium dihydrogenphosphate, NaH2PO4 = 0.80 mol  Moles of sodium hydrogenphosphate, Na2HPO4…

Q: Suppose you are asked to prepare a buffer solution for an upcoming experiment using stock solutions…

A:

Q: A buffer solution contains 0.202 M of a weak acid and 0.224 M of its conjugate base. The K, of the…

A: Buffer solution is a solution whose pH does not changes on standing as well as on addition of small…

Q: Consider a solution of 0.0150 M Na2C6HgO6 (sodium ascorbate), answer the following questions:…

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Q: 1. The ionization constant (Kb) of aniline (C6H5NH2) is 2.35 x 10^-5. If 7.285 grams of aniline is…

A: We can easily calculate the equilibrium concentration of the species by constructing an ICE table.…

Q: CH, NH, is a weak base (Kp = 5.0 x 10-"), so the salt CH, NH, NO, acts as a weak acid. What is the…

A:

Q: 50.0 ml of 0.1 M NaOH is added to 100.0 ml of 0.2 M HCN (Ka=6.2x10-10). What is the pH of the…

A: A buffer solution is a mixture of weak acid and its conjugate base or weak base and it's conjugate…

Q: At 22 °C, an excess amount of a generic metal hydroxide, M(OH),, is mixed with pure water. The…

A: Given ph is more than 7  Convert in poH term.

Q: What is the pH of the resulting buffer solution when 25mls of 0.10 M NaH is added to 25mls of 0.200…

A: pH of the buffer solution is calculated by using Henderson equation, it is,

Q: A buffer solution contains 0.19 mol of hypochlorous acid (HClO) and 0.63 mol of sodium hypochlorite…

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Q: If a buffer solution contains 1.6 M acetic acid and 2.3 M sodium acetate, what is the pH of the…

A: Given  ka (Ionisation constant)                 = 1.8 × 10-5 Concentration of CH3COOH         = 1.6…

Q: At 22 °C, an excess amount of a generic metal hydroxide, M(OH),, is mixed with pure water. The…

A: M(OH)2  ↔  M2+   +  2 OH-Expression for Ksp ,Ksp = [M2+] [OH-]2  Find out the individual…

Q: t 22 °C, an excess amount of a generic metal hydroxide, M(OH),, is mixed with pure water. The…

A:

Q: If the solubility of silver carbonate (Ag2CO3) is 1.3 x 10-4 mol/L, what is the concentration of the…

A: