A 0.251 M aqueous solution of monoprotic weak acid is measured to have a pH = 5.36. What is the value of Ka for this acid?  Enter your answer in exponential format using a capital "E"  (example 1.23E-4) and no units (value ± 4%). The answer is 7.59*10^-11 but I would like an explanation please.

Q: An acid (HA) dissociates as follows: HA – H* + A minus Arrow should be interpreted as an equilibrium…

A: The equilibrium reaction given is, => HA --------> H+ + A-  Given : Initial concentration of…

Q: The equilibrium constant, Ka, for a monopratic acid (propionic acid) is 1.3 ×10^-5. Which of the…

A:

Q: Calculate the pH of 0.035 M  aqueous solution of acetic acid (CH3COOH). Ka (CH3COOH) = 10-4.8 Group…

A: Concentration of acetic acid solution = [CH3COOH] = 0.035 MKa for acetic acid (CH3COOH) = 10-4.8pH…

Q: The pH of a 1.4M solution of acetic acid (HCH,CO,) is measured to be 2.30. Calculate the acid…

A: Given- pH=2.30 Concentration of acetic acid= 1.4M

Q: Can you please further explain to me what I have to do to find the theoretical pH? I’ve prepared a…

A: Given question to calculate the pH of acetic acid solution.

Q: Conside following data on some weak acids and weak bases: acid base K. name formula name formula…

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Q: The pH of a 0.24 M solution of dimethylamine is 12.51. Calculate the Kb value for dimethylamine (4.4…

A: Hello. Since more than one question has been asked, the first question will only be solved in this…

Q: What is the pH of this solution?

A: Ka is the ratio of  product of concentration of products raised to their stoichiometric coefficient…

Q: find PH for part C and D Part C 0.085M in HF(K = 6.8 × 104) and 0.225M in HC H₂O (K = 1.3 × 1010)…

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

Q: If we used H2C4H4O5 as the weak diprotic acid, which of the four species, H2C4H4O5, HC4H4O5^-,…

A: Given that, H2C4H4O5 is a weak diprotic acid & the four species are H2C4H4O5, HC4H4O5-,…

Q: If 0.10 M aqueous solutions are prepared of each of the following acids, which produces the solution…

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Q: My Grades - BIOL111ASP2020 MB Canvas Login at Mary Baldwin Ur X O Chemistry 121 101 Chem101 Question…

A: A strong acid shows complete dissociation to respective anion and H3O+whereas a weak acid can only…

Q: solution is prepared at 25°C that is initially 0.41M in chloroacetic acid (HCH2ClCO2) , a weak acid…

A: Given,  Concentration of Acid = 0.41 M Concentration of Salt = 0.0821 M Ka = 1.3 ×10-3 pKa = 2.89 As…

Q: Be sure to answer all parts.   The pH of a 0.062 M weak monoprotic acid is 3.37. Calculate the Ka of…

A: The pH of the acid is 3.37 The concentration of hydrogen ions can be determined as follows: pH  =…

Q: Construct the expression for Ka for the weak acid, CH,COOH. CH,COOH(aq) + H,O(1) = H,O*(aq) +…

A: Given data :

Q: Answer the following questions about weak acids. Use the K. values in the following table to help…

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Q: Selected acid base/base pair: Propanic Acid (CH3CH2COOH) / Sodium Propanoate (NaCH3CH2COO) with Ka =…

A: Ka of propionic acid = 1.4 x 10-5 Propionic acid is weak acid and sodium propionate as conjugate…

Q: An acid (HA) dissociates as follows: HA – H* + A minus Arrow should be interpreted as an equilibrium…

A:

Q: The pH of a 0.052M solution of acrylic acid (HC,H,CO,) is measured to be 2.77. Calculate the acid…

A: GivenpH = 2.77pH = -logH+2.77 = -log H+H+ = 0.00169 M[H+] = 1.7 * 10-3 M

Q: A 0.035 M solution of a weak acid has a pH of 2.21. Calculate the acid ionization constant (Ka) of…

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Q: Without doing any calculations, which of the following acids, if in solutions of equal…

A: 11.  Ka is the ratio of  product of concentration of products raised to their stoichiometric…

Q: The pH of a 0.69M solution of alloxanic acid (HC4H₂N₂O) is measured to be 3.41. Calculate the acid…

A: pH = 3.41 Concentration  (c) = 0.69M Ka =?

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: sure your answer has the correct number of significant digits. Calculating the pH of a strong base…

A: Given :  Mass of Barium hydroxide = 216. mg  Volume of solution = 190. ml

Q: A weak monoprotic base has a Kb = 9.11 × 10−10. Calculate the Ka for the conjugate acid of this…

A: The relationship between Ka and Kb is: Ka × Kb = KwKa × Kb = 1.0×10-14

Q: Considering a molecular orbital diagram for a diatomic molecule, which of the following bond orders…

A: Option d. According to molecular orbital theory the bond order of a diatomic molecule is given by:…

Q: The pH of a 1.1M solution of propanoic acid (HC,H,0,) is measured to be 2.41. Calculate the acid…

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Q: The pH of a 0.80 M solution of propanoic acid (HC_3H_50_2) is measured to be 2.48. Calculate the…

A: The objective of this question is to calculate the acid dissociation constant of propanoic acid.

Q: Determine the pH of an aqueous solution that is 5.93×10-5 M in NaOCl. Set up relevant equilibrium…

A: The question is based on the concept of pH of the solution.  It is defined as a negative logarithm…

Q: The weak acid HXO2 has a dissociation constant of Ka = 8.50 × 10-10.  A lab worker prepares of 0.600…

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Q: The weak acid HXO2 has a dissociation constant of Ka = 4.50 × 10-10.  A lab worker prepares of 1.500…

A:

Q: An acid (HA) dissociates as follows: HA → H* + A minus Arrow should be interpreted as an equilibrium…

A: Acid dissociation constant is commonly known as Ka , it measures the strength of acid in solution.

Q: An acid HA has a Ka of 1.00 x 10-7. Calculate the pH of a 0.100 M solution of its conjugate base.…

A: Given: Concentration of conjugate base of weak acid HA i.e. A- = 0.100 M And Ka of HA = 1.00 × 10-7…

Q: A0.450 M solution of a weak acid HA has pH=4.72. Calculate Ka for this acid. Express your answer in…

A: Given :-  pH of solution = 4.72  Concentration of weak acid = 0.450 M  To calculate :-  Ka for the…

Q: The pH of a 0.46M solution of propanoic acid (HC,H,O,) is measured to be 2.60. Calculate the acid…

A:

Q: Morphine (C17H1903N) is very effective at relieving intense pain. Calculate the pH of a 0.00115 M…

A: Concentration of morphine = 0.00115 M  Value of Kb = 8.0 × 10-7

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.