A 0.200 M solution of nitrous acid (HNO2) had a pH of 2.07. What is the Ka value for nitrous acid.

Q: What is the pH of a 3.50 M solution of NH4CI (Ká of NH3= 1.8 x 105)?

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Q: Carbonic acid, H,CO, is a diprotic acid with Ka1 = 4.3 × 107 and Ka2 = 5.6 × 1011. What is the pH of…

A: H2CO3 ⇌HCO3−  +   H+.........     ka1= 4.3x10-7 HCO3− ⇌CO3-2 ​+   H+..........    Ka2=5.6x10-11ka1…

Q: 1) A 0.45M aqueous solutionof creatine, (C4H9N3O2), has a pH of 1.49. Calculate the value of the…

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Q: For H2CO3, Ka1 = 4.3 × 10–7, Ka2 = 4.7 × 10–11. What is the pH of a 0.36 M solution of carbonic…

A: We have to predict the pH of 0.36 M of carbonic acid .

Q: Calculate the pH of a 0.30M solution of sodium acetate (NaCH3COOo) given that the Ka of acetic acid…

A: Formula for calculating pH of as solution of a salt made from a weak acid and a strong base: pH = 7…

Q: Calculate the pH at 25°C of a 0.45 M aqueous solution of oxalic acid (H2C2O4). (Ka1 and Ka2 for…

A: We have to calculate the pH value.

Q: A 0.495M solution of nitrous acid, HNO2, has a pH of 1.83. Calculate the value of Ka for nitrous…

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Q: The pH of a solution that is 0.5 in MA and 0.3 in HA is 5.40; determine the pKa of the acid.

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Q: What is the pH of a 0.40 M solution of sodium nitrate, NaNO2 ? The pKa for nitrous acid (HNO2) is…

A: Base dissociation constant Kb is utilized to determine the basic nature of a solution. It refers to…

Q: The pH of a 0.05 M acid solution is 1.4. What is [H] in that solution? If the K, for the acid is 3.3…

A: We know that pH is the negative logarithm of H+ ion concentration. that is  pH = – log[H+] ⇒[H+] =…

Q: Nitrous Acid (HNO2) has a Ka value of 5.6x10–4. Calculate the pH of a solution that is 0.00298 M…

A: pH = -log[H+] For a weak acid solution: [H+] = (Ka x C)1/2 Where, C = molarity of acid

Q: 1. How many grams of Ca3(PO4)2 will be needed to prepare 500.0 mL of a 0.161-M solution of…

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Q: Fill in the left side of this equilibrium constant equation for the reaction of benzoic acid…

A: The Equilibrium constant for a reaction   A + B ⇔ C + D   Can be written as  K = [C][D][A][B],…

Q: a general chemistry student measured the pH of a 0.510 M aqueous solution of nitrous acid to be…

A: Here we are required to find the dissociation constant for weak acid nitrous acid

Q: Calculate the pH of a solution prepared by mixir (Ka-6.46 x 105) with 5.00 mL of 0.200 M NaO…

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Q: Carbonic acid, H₂CO₃ is a diprotic acid with Ka1 = 4.3 × 10⁻⁷ and Ka2 = 5.6 × 10⁻¹¹. What is the pH…

A: pH of a 0.48 M solution of carbonic acid = 3.35

Q: Propionic acid, CH3CH2COOH, has a Ka = 1.34 x 105. If 10.00 mL of 0.080 M propionic acid is mixed…

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Q: Calculate the pH of a 0.010-M solution of iodic acid (HIO3, Ka = 0.17).

A: Molarity of Solution = 0.010M Ka of Acid = 0.17 We have to find the pH of the solution of iodic…

Q: What is the pH of a mixture of 0.042 M NaH2PO4 and 0.058 M Na2HPO4?

A: Given : Concentration of NaH2PO4 = 0.042 M Concentration of Na2HPO4 = 0.058 M

Q: 1,2-diaminoethane, H2N-CH2-CH2-NH2, is used extensively in the synthesis of compounds containing…

A: The dissociation reaction is given as, H2N-CH2-CH2-NH2 + H2O →H2N-CH2-CH2-NH3+ + OH-

Q: A weak monoprotic acid, HA dissociates by 2.416 % and has a pH of 3.61. Calculate the Ka value for…

A: percent dissociation of HA is 2.416% pH = 3.61

Q: Calculate the pH of a solution that is a mixture of 0.030M HNO3, 0.55M CH3COOH, and 0.015M HI. Ka…

A: Given data : HNO3 = 0.030 M HI = 0.015 M CH3COOH = 0.55 M

Q: Calculate the pH values of the following solutions: a) a 0.1 M solution of protonated methylamine…

A: Given data: Concentration of methylamine = 0.1M Concentration of HCOOH  = 0.3M Concentration of…

Q: Calculate the concentration of all species in a 0.470 M solution of H2SO3. The acid ionization…

A: The H2SO3 solution contains the following species,

Q: A 0.100 M solution of nitrous acid (HNO2) had a pH of 2.07. What is the Ka value for nitrous acid.…

A: We are given Nitrous acid and its pH. We have to find Ka. Concentration of nitrous acid = 0.1 M

Q: When 2.0 x 10-2 mole of nicotinic acid (a monoprotic acid) is dissolved in 350. mL of water, the pH…

A: Nicotine is a weak monoprotic acid so it dissociated in less amount. So we can denotes it by HA .

Q: Calculate the pH of a 0.325 M solution of a weak base whose conjugate acid has a pka-5.155.

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Q: Carbonic acid, H₂CO₃ is a diprotic acid with Ka1 = 4.3 × 10⁻⁷ and Ka2 = 5.6 × 10⁻¹¹. What is the pH…

A: The carbonic acid is a diprotic acid. The major release of hydrogen ions occurs in the primary…

Q: Calculate the pH of a 0.0101 M aqueous solution of formic acid (HCOOH, Ka = 1.8E-4). pH =

A: For weak monoprotic acid ( HCOOH) : pH = 0.5 x (- log Ka - log C ) pH = 0.5 x ( - log 1.8 x 10-4 -…

Q: What is the pH of a solution with a fluoride concentration of 0.20 M ? The Kb for F– is 1.47×10-11 .

A: In order to find the pH of the solution we first write down the given data: Fluoride concentration=…

Q: Part II. Arrange the following compounds in order of increasing basicity. 7. NazO, Rb2O, K2O 8.…

A: Ans. Part II Arrangement of the given compounds in order of increasing basicity: (7)  Na2O <…

Q: The acid dissociation reaction for the weak acid butyric acid, HC4H¬O2 is given below. Its Ka is…

A: The dissociation reaction given is Assuming y concentration of HC4H7O2 dissociates as per the…

Q: Which of the following salts would produce the most acidic 0.10 M aqueous solution? FeCl, KF, KNO,…

A: FeCl is the right answer. Whichever is the stronger acid will be the dominate factor in determining…

Q: What is the pH of a solution that is 0.05M in ethylamine and 0.08M in its chloride salt (pKa=10.8)

A: pH of a solution =?    [ C2H5NH2 ] = 0.05 M    [ C2H5NH3+ ] = 0.08 M Acid dissociation constant :…

Q: Given the following compounds: H2S (34.065); NaHS (56.065); Na,s (78.065), calculate the pH of a…

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Q: Calculate the pH of a solution prepared by dissolving 0.040 moles of sodium nitrite (NaNO2) in 200…

A: When HNO2 and NaNO2 are mixed, they form buffer solution HNO2/NO2-. And the pH of a solution is…

Q: Barbituric acid, HC4H3N2O3, is used to prepare various barbiturate drugs (used as sedatives).…

A: Given data: The concentration of Barbituric acid solution [HC4H3N2O3]=0.10 M. The acid dissociation…

Q: 22:b) Solution A has a PH = 8.94 and Solution B has a [OH] = 4.5 x 10+ M. Which solution is more…

A: Here is the solution

Q: What is the pH of a 0.15M solution of potassium nitrate? (The Ka value for nitrous acid is 4.0 x…

A: Considering the given solution to be 0.15 M potassium nitrite, we have solved further.

Q: A 2.00 L aqueous solution of a monoprotic weak acid, HA, with a concentration of 0.750 M has a pH of…

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Q: The following reaction has a AG° value of +8.43 kJ/mol at 25 °C. HA(aq) + H20(1) =H;0*(aq) +A (aq)…

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Q: What is the pH of a solution of 0.0745 M NACH3O2 ? Ka = 1.8 x 10

A: Given: Concentration of NaC2H3O2, [NaC2H3O2]= 0.0745M Ka = 1.8 x 10-5

Q: A 2.00 L aqueous solution of a monoprotic weak acid, HA, with a concentration of 0.105 M has a pH of…

A: Since pH = -log[H+] = -log[H3O+] Hence substituting the values we get  2 = -log[H3O+] => [H3O+] =…

Q: A buffer solution is 0.402 M in NaH2PO4 and 0.318 M in Na2HPO4. If Ka for H2PO4- is 6.2 x 10 -8,…

A: The solution has NaH2PO4 which will dissociate completely into ions Na+ and H2PO4-  Hence…

Q: Calculate the pH of a 0.300 M solution of lactic acid, for which the Ka value is 1.40 x 104. A. 8.67…

A: Lactic acid is a weak acid. Given data is: concentarion of solution = 3.00 M Ka=1.40×10-4 Now, next…

Q: 6. Calculate pH for the 0.05 M Ca(OH)2 and 0.01M HCl and explain the natures of the solutions after…

A: Ca(OH)2 pH-13 HCl pH- 2

Q: Show the calculations to demonstrate that 2% AgNO3 is approximately 0.1M in Ag+ ions.

A: Given:the given concentration of AgNO3 must be in w/vconcentration of AgNo3 (w/v)=2%The formula for…

Q: What is the pH of a 0.340 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

A: The salt given is Ca(NO2)2  Since the salt is made up of strong base cation from Ca(OH)2 and anion…

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.