he pH of the solution formed by mixing 50 ml of 0.1 M CH3COOH solution (Ka = 1.8 × 10-⁵) with 45 ml of 0.1 M NaOH solution is: a) 4.74 b) 5.7 c) 7.5 d) 9

Q: 5. The pK,'s for phosphoric acid represent the following ionizations: H;PO4 2 H2PO4 + H* pK = 2.14…

A: Chemical reaction between H3PO4 and NaOH is:   H3PO4+3NaOH→Na3PO4+H2O

Q: How many moles of HA would need to be added to 481 mL of 0.816 M NaA to produce a solution with a pH…

A:

Q: (Q11) lodic acid (HIO3) is a relatively strong weak acid (Ka = 0.17). What will be the equilibrium…

A:

Q: A solution that is 6.0×10−2 M in potassium propionate (C2H5COOK or KC3H5O2 ) and 8.0×10−2 M in…

A: A solution given is 6.0×10−2 M in potassium propionate (C2H5COOK or KC3H5O2) and 8.0×10−2 M in…

Q: Methylamine is a weak base for which Kb is 4.4 × 10-4 . Calculate the pH of a solution made by…

A: The pH of a solution depends upon concentration of hydrogen ion but here solution will be basic so…

Q: Determine the pH of a 1.0M solution of sodium acetate (NaC2H3O2). Ka = 1.8x10-5 for acetic acid.

A: Dear student,  As you have asked multiple question but according to guidelines we will solve first…

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0176 M solution. The pH of the…

A: Given, Concentration of weak acid (C) = 0.0176 M pH of solution = 2.47 Dissociation constant (Ka) =…

Q: Calculate the pH of a solution when 21.0 mL of 0.050 M hydrazine (N2H2, Kb=8.9E-7) is titrated with…

A: pH of a weak base titration with strong acid can be determine using Henderson hasselbalch equation.

Q: Halpinious acid, H2JHO3, is a weak diprotic acid with Ka1 = 2.40 x 105 and Ka2 = 4.79 × 10-11 at…

A: Given Ka2 <<<< Ka1 so, [H+] = Ka1.C [H+] = 2.40 × 10-5×0.500 = 3.46 × 10-3 M  pH = -log…

Q: of

A: According to the question, we need to calculate the pH of the following solution.    A. Here, pOH =…

Q: The pH at 25 °C of an aqueous solution of the sodium salt of α-naphthol (NaC10H7O) is 11.23.…

A: pOH is used to determine the concentration of hydroxide ion. The expression of pOH is shown below:…

Q: What is the pH of a 80.0 mL solution which is 0.23 M in IO and 0.47 M in HIO? The Ka for HIO is 2.3…

A: When a weak acid(eg HIO) mixed with its conjugate base (ege IO-) they form a buffer solution. pH of…

Q: The base Ca(OH)2 is almost insoluble in water , only o 25 g can be dissolved in 0.5 L of water at 25…

A: Given : Mass of Ca(OH)2 dissolved = 25 g And volume of solution = 0.5 L…

Q: : Calculate the pH of a 0.08M HCN solution. Ka is 7.2 x 10-10 5.12 6.00 7.60 7.26 None of these

A:

Q: Furoic acid (HC5H3O3) has a Ka value of 6.76 * 10-4 at 25 °C. Calculate the pH at 25 °C of a…

A: Buffers are the solutions that resists the change in pH on addition of small amount of acid or base.…

Q: A 0.144 M solution of HA has a pH of 2.26 at 25°C. What is the value of Ka for HA? (the answer…

A: Given that, a 0.144 M solution of HA has a pH of 2.26 at 25°C. I.e. concentration is C = 0.144 M.…

Q: What is the pH of the resulting solution if 45.00 mL of 0.10 M acetic acid is added to 10.00 mL of…

A: Given data contains, Volume of acetic acid is 45.00mL. Molarity of acetic acid is 0.10 M. Volume of…

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

A:

Q: What is the pH of a 40.0 mL solution that is 0.13 M in CN¯ and 0.27 M in HCN? The K, for HCN is 4.9…

A:

Q: Calculate the Ka of a 0.10M acid solution which is 8.1% ionized

A: Given : concentration = 0.1 M Percent of dissociation = 8.1% Ka = C × ( degree of dissociation) 2

Q: 6) Calculate the pH of a solution formed by mixing 250.0 mL of 0.900 M NH4C1 with 250.0 mL of 1.60 M…

A:

Q: Calculate the pH of a mixture that contains 0.20 M of HCOOH and 0.16 M of HC,H,O. The Ka of HCOOH is…

A:

Q: The Kb of dimethylamine [(CH3)2NH] is 5.90×10-4 at 25°C. Calculate the pH of a 1.15×10-3 M  solution…

A:

Q: dict the pH range of aqueous solutions of the following salts: KNO3, KHCO3, NH,F, and NH¼Br,…

A: The question is based on the concept of salt hydrolysis. We have to identify the nature of the salts…

Q: 2,What is the pH of the solution with  hydronium ion concentration of 6.3 x 10-12 M? Group of…

A: We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…

Q: What is the pH of a 0.70 M NAOH solution with a volume of 50.00 mL after 30.00 mL of 0.35 M solution…

A:

Q: The Kb of dimethylamine [(CH3)2NH] is 5.90×10-4 at 25°C. Calculate the pH of a 1.10×10-3 M  solution…

A:

Q: Calculate the pH of a solution prepared by mixing 100.0 mL of 0.100 M NH3 with 200 mL of 0.100 M…

A: Dissociation constant value for particular acid/base always depicts how rapidly any acid/base gets…

Q: Anisic acid (Ka=3.38x10^-5) is found in anise seeds and is used as a favoring agent. For a 0.867 M…

A: From given concentration of anisic acid = 0.867 M  So from that  All given categories like  H+, OH-,…

Q: pH

A:

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0114 M solution. The pH of the…

A: Hello. Since your question has multiple parts, we will solve the first question for you. If you want…

Q: 1. Calculate the pH of a solution with [OH'] = 3.86×10-5. 2. A 10.0 mL sample of 5.00M HCl is…

A: Question 1 :-  We have to find out the pH of the given solution for this first we have to calculate…

Q: A solution of dimethylamine is prepared by dissolving 1.3525 grams of dimethylamine in 25 mL ethanol…

A: Dimethylamine reacts with HCl as: CH3NHCH3+HCl→CH3NH2+CH3+Cl-

Q: -2.15 =,75 0.4 3x10-3 10. If 600 ml of a .7M HC2H3O2 is reacted with 800 ml of a .5M solution of…

A:

Q: HCIO is a weak acid (Ka=4.0*10^-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

A: At 25° C strength of NaOCl is 0.018 M and given Ka of acid is 4×10-8  We have to calculate the pH of…

Q: A 0.200 M formic acid (HCOOH) solution is tested with a pH meter at 25°C and found to have a pH of…

A: we have to calculate the value of Kb for formate ion

Q: In a particular solution, acetic acid is 18% ionized at 25°C. Calculate the pH of the solution and…

A: The species acetic acid will be described as the types of weak acid because having a smaller acid…

Q: Phosphoric Acid (H3PO4) has pKa values: 3.13, 4.76, 6.40. What is the pH made by dissolving 0.200…

A: When a substance increases the concentration of the hydrogen ion in an aqueous solution, then the…

Q: What is the approximate pH of a solution formed by mixing 45.0 mL of 0.10M HNO3, 50.0 mL of 0.20M…

A: Given: The volume of HNO3=45.0 mL  Molarity of HNO3=0.10M  Volume of HCl=50.0 mL  Molarity of…

Q: Which of the following solutions at 25°C will have the lowest pH value? A 0.15 M Na2S04 (Ka of H2SO4…

A:

Q: Which of the following solutions would be expected to have a pH of 7.00? Weak Ka Kb Base < 10-10…

A: When a salt is formed by reaction of strong acid and strong base , then the salt is neutral salt and…

Q: An aqueous solution is prepared by mixing 50 mL of 2.0M KHPO4 and 25 mL of 2.0M K2HPO4 ,to a final…

A: The question is based on the concept of PH  calculations.   pH is defined as negative logarithmic of…

Q: 4. By the middle of this century, the partial pressure of carbon dioxide (CO2) in Earth’s atmosphere…

A:

Q: 3. Give the pH of the following: 2 mL of 15.4 M stock solution of HCl is mixed with water to а. make…

A:

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: Assume H2SO4 is a completely strong acid, and forms 2 H+ and an SO4-2 when dissolved in water.   A…

A: An acid is a substance that gives H+ ions in its solution whereas a basic substance gives OH- ions…

Q: the pH of modern rain water (= 5.61) in equilibrium with air at 25°C and a total pressure of 1…

A:

Q: Ка 3 1.76 х 10-5 for HC2H302 What is the pH of this solution? Table 1 2 Solution Buffer solution C…

A:

Q: You have 50.0 mL 0.10 M N3PO4 to whihc you add 50.0 mL 0.19M NaH2PO4. What is the pH of this…

A: Calculation of no. of mol of H3PO4: No. of mol=Molarity×Volume=0.10 mol/L×50.0×10-3L=0.005 mol…

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.