How many ml of 0.1 M HCl must be added to 100.0 ml of 0.2 M NaCN (Kb=1.6x10-5) to achieve a pH of 8.2?

Q: The Ksp for In(OH)3 is 1.3 x 10-37.…

A: Hello. Since your question has multiple sub-parts, we will solve the first three sub-parts for you.…

Q: What is the Ph of a 0.23 M triethylamine (C2H5)3N solution? Kb for triethylamine is 5.3 x 10^-4.…

A: pH = -log [H+] pOH = -log [OH-] Also pH + pOH = 14

Q: Ka for hypochlorous acid HCIO is 3.0 x 10-8. Calculate the pH after the addition of 15.0o mL of…

A: Initial moles of HClO = Molarity ×Volume = 0.100 M × 40.0 mL = 4mmoles Initial moles of NaOH =…

Q: How many grams of NaIO (Kb (IO-)=5x10-4 ; MW=213.9 g/mole) must be added to 40.0 ml of 0.1 M HCl to…

A: pOH = pKb + log [NaIO]/[HOI] pH = 14 - pOH

Q: How many moles of B (weak base) would need to be added to 524 mL of 0.209 M BHCl (the acidic salt)…

A:

Q: Calculate the hydronium ion concentration and the pH when 35.0 mL of 0.45MN*H_{3} is mixed with 35.0…

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Q: he Ka of acetic acid is 1.8 x 10 -5. Calculate the pH of a solution which is composed of 0.250 M HCH…

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Q: What is the hydronium and hydroxide ion concentration of pure water at 100°C? (Kw = 49 x 10-14)

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Q: What is the pH of an aqueous solution that consist 40.0 mL of 0.050 M HCl and 30.0 mL solution…

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Q: acid has a Ka of 1.8 x 10-5. Calculate the pH at the point when 30.00 mL of 0.150 M NaC2H3O2 is has…

A: The solution can be provided as:

Q: Using tabulated Ka and Kb values, calculate the pH of the following solution. Answer to 2 decimal…

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Q: Determine the pH of solution if 0.085g of acetylsalicylic acid, HC9H7O4, (Ka = 3.0 x 10-5) is…

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Q: 8) What will be the pH (aq., 25 oC) of 250.0 mL of a solution of 0.821 M HCOOH and 0.909 M HCOOK,…

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Q: Anilinium chloride (C6H5NH3Cl) is a weak acid (Ka = 2.4 x 10-5). A sample of anilinium chloride…

A: “Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

Q: Calculate the pH of a solution formed by mixing 500.0 mL of 0.075 M CH3NH3Cl with 200.0 mL of 0.10 M…

A: Given: Volume of CH3NH3Cl = 500 mLMolarity of CH3NH3Cl = 0.075 MVolume of CH3NH2 = 200 mLMolarity of…

Q: What is the pH of an aqueous solution with .5 M NH3 & .45 M NH4Cl?  Kb=1.78 x 10-5

A:

Q: Dilution. 100 mL100 mL of a solution of hydrochloric acid with pH 5.0 pH 5.0 is diluted to 1 L1 L.…

A: pH of a solution is equal to the negative logarithm of hydrogen ion concentration. Using this…

Q: at 95 ℃ water has an autoionization constant (Kw) of 4.518 X 10-13. Determine the ph of pure water…

A: Given :- Kw at 95°C = 4.518 × 10-13  To determine :- pH of pure water at 95°C

Q: A generic weak acid was prepared and has a concentration of 0.471 M. Its Kb value is 4.91x10-10.…

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Q: When added to pure water in equal quantities, a Base with a Kb = 2.4 x 10-8 will cause greater pH…

A: when base B is added to water it abstract hydrogen ion from water to form BH+  the reaction  is…

Q: Calculate the pH of a 50 mL solution of 0.20 M oxalic acid (pKa1 = 1.25, pKa2 = 4.27) by mixing 50…

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Q: The Ka of hydrofluoric acid (HF) at 25.0 °C is 6.8 × 10-4. What is the pH of a 0.15 M aqueous…

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Q: What is the pH of a solution containing 1.50 M Acetic acid (CH3COOH) (Ka = 1.8 X 10-5) and 2.5 M…

A: Solution, which resist in pH change value upon addition of small amount of strong acid or base (less…

Q: Determine the pH of a 0.62 mol L-1 NH4NO3 solution at 25oC. The Kb for NH3 is 1.76 x 10-5. Select…

A: Ammonium  nitrate is the salt of weak base and strong acid. When it is dissolved  in water it…

Q: Determine pH of solution containing 0.210 M C6H7NH3Cl. (Kb  of C6H7NH2 is  4.50 x 10-6)     A.…

A:

Q: Determine the pH of a solution made of 0.0082M H3PO4 and 0.0046M Na2HPO4. (Ka of H3PO4 = 7.11 x…

A: Balance chemical equation:                                   H3PO4 + Na2HPO4  ----->   2NaH2PO4…

Q: 100.0 ml of a 0.3 M solution of an unknown monoprotic weak acid has a Ka=1x10-6.  What mass of NaOH…

A: Volume of weak monoprotic weak acid = 100ml Molarity of weak monoprotic weak acid = 0.3M Ka = 1 x…

Q: The pH of a solution made from a 0.75 M acetic acid solution and a 0.54 M sodium acetate solution is…

A:

Q: What is the pH of 100.0 mL of 0.10 M HNO;? nooulos M 005.0s ai nois 01 x 02.1 g CH'COOH What is the…

A: pH = -log [H+]

Q: An unknown weak base with a concentration of 0.170 M has a pH of 9.26. What is the Kb of this base?…

A: Weak base dissociated less in solution

Q: How many grams of NaOH (MW=40.0 g/mole) do you need to add to 50.0 ml of a 0.2 M weak acid HA…

A: Given data contains, Concentration of HA is 0.2 M. Volume is 50.0 mL. Ka is 4×10-6. The moles of HA…

Q: What is the pH when 24.5 mL of 1.00 M NaOH has been added to 25.0 mL of 1.00 M CH3COOH…

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Q: If 50 ml 0.40 M HCl  is added onto the 40 ml 0.15 M NaCN solution, what is the final ph?

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Q: Im doing a lab report on the creation of soap through the saponification process, and am currently…

A: Soap is made by saponification reaction in laboratory. In this method, soap is made by reacting…

Q: What is the pH when 20.0 mL of 0.10 M sodium hydroxide is added to 40.0 mL of 0.15 M HIO (Ka = 2.0 ×…

A: Given: 20 ml of 0.10 M NaOH (Base) 40 ml of 0.15 M HIO  (Acid) Ka of HIO = 2.0 x 10-11 we need to…

Q: Suppose you have just added 50.0 ml of a solution containing 0.0400 moles of weak acid HA to 500.0…

A: When weak acid is titrated with strong base, the resultant solutionwill have unionized acid and salt…

Q: The buffering range for HC2H3O2 (Ka =1.8 X 10-5) would be approximately __________.     pH 2-4…

A: Buffer can resist the change of pH. Ka of HC2H3O2 = 1.8 ×10-5

Q: Calculate how much of each solution you need to take to prepare 1 L of buffer solution with a pH of…

A: The question deals with the concept of Buffer preparation. by adding suitable amount of sodium…

Q: The pH after adding 21.0 mL of 1.0 M NaOH to 25.0 mL of 1.0 M HCl is   0.087   0.16   0.80   1.1

A: The pH of a solution indicates the basicity or acidity of a solution, which is calculated using the…

Q: Calculate the pH of a solution of 0.01 M NaF, given Kb for F- = 1.4 x 01-11. Group of answer…

A: NaF <---> Na+ + F-  ICE Table –       F-   +     H2O <---> HF    +    OH- I   0.01…

Q: 1. calculate the pH of a solution obtained by mixing 30.4 mL of 0.03 M HCL with 31.4 mL of o.1 M…

A: SOLUTION 1. Here both HNO3 and HCl are strong acid, total proton concentration is the sum of the…

Q: A 50.0 mL solution of the weak acid HA (Ka = 1.00 × 10-6) has a pH of 4.000. What volume of water…

A: Given, Initial volume of HA  = 50.0 mL The initial pH value of HA at 50.0 mL = 4.000 The final pH…

Q: What is the pH of 0.541 M dimethylammonium iodide, (CH3)2NH21? At 25°C, the Kb of (CH3)2NH is 5.9 x…

A: Dimethylammonium iodide is a salt of a strong acid, HI, and weak base, (CH3)2NH. So, in this case,…

Q: Calculate the pH of 50.0 mL of 0.250 M oxalic acid (HOOCCOOH) upon addition of 31.9 mL of 0.500 M…

A: Answer: In this question we have to find out the pH of a buffer solution made from the mixture of…

Q: Calculate the pH of hydrolysis of 0.500M NaF in water. (Ka=8.1x10^-4)

A: A strong base and weak acid react to form salt and water. The salt will be basic in nature and the…

Q: Determine how much of each acid and conjugate base are needed to add to a final volume of 500ml of…

A: The preparation of buffer is governed by Henderson Hasselbach equation. pH=pKa + log[conjugate…

Q: What is the pH of a solution in which 21.65 mL of 0.28 M HNO3 is added to 9.95 mL of 0.067 M…

A: HNO3 is strong acid Ba(OH)2 is strong base.

Q: Calculate the theoretical pH of each solution. a. 0.200 M sodium bicarbonate Carbonic acid: pKa1 =…

A: #(a): [NaHCO3(aq)] = 0.200 M or 0.200 mol/L For HCO3-(aq), kPa2 = 10.25 and pKb2 = 14-pKa1 = 14 -…

Q: the solution of 2.50 L of a 0.250M CH3CO2H has a pH of 4.20, what is the pH if you add 20.0 mL of…

A: At equilibrium,                              CH3COOH  ⇌  CH3COO-  +  H+  The pH of this solution can…

Q: How many moles of B (weak base) would need to be added to 524 mL of 0.209 M BHCl (the acidic salt)…

A:

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.