2. If 25.00 mL of a 0.09864 M CH;COOH (Ka = 1.8 x 10-5) solution is titrated with a 0.1027 M NaOH solution, what will be the pH in the following conditions?

Q: A 0.035 M solution of a weak acid (HA) has a pH of 4.88.What is the Kₐ of the acid?

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Q: a When you add solid sodium oxalate, Naz C2 04, to 50.0 mL of 0.015 M oxalic acid, H2 C204, what…

A:

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

A: Ka of HClO = 4.0 × 10-8 Concentration of the solution of NaClO = 0.089 M pH =?

Q: Calculate 3OH-4 and pH for 1.00 mL of 0.175 M NaOH diluted to 2.00 L

A: The formula used to calculate pH: pH=-log(H+). Given data: Concentration of NaOH is 0.175M. Volume…

Q: A 0.120 M solution of a weak acid (HA) has a pH of 3.29.  a) Calculate the acid ionization constant…

A: Given,Concentration of a solution of weak acid, HA = 0.120 MpH of the solution = 3.29The…

Q: What will be the pH of a solution when 100.0 mL of 0.100 M NaOH is reacted with 9 mL of 1.00 M…

A: According to the question, we need to calculate the pH of the solution when 100 ml of 0.100 M NaOH…

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: What is the pH of 3.78 *10^-2 M nitric acid in aqueous solution ?

A: Concentration of hydronium ion H3O+ present in the solution is known as the pH of the solution.

Q: What is the pH of a 0.1055 M CH3COOH solution (Ka = 1.75 × 10−5)?

A: Given concentration of CH3COOH = 1.75 × 10-5

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

A: Given data; Ka=4×10-8Also, Kw=Ka×KbAnd,Kw=1×10-14 Consider the dissociation of given weak acid as;…

Q: What is the pH of a 0.17 M weak acid solution? The KA of the weak acid is 2.1 x 10-5.

A: Given :-  Initial concentration of weak acid = 0.17 M  Ka for acid = 2.1 × 10-5  To be calculated :-…

Q: How many moles of NH3 must be dissolved in water to give 813.0 mL of solution with a pH of 11.15? Kb…

A: The value of Kb for the given weak base is = 1.8x10-5 The concentration of the base solution is =?…

Q: If the Ka of a monoprotic weak acid is 3.4 × 10-6, what is the pH of a 0.30 M solution of this acid?

A: The dissociation of a weak acid is written as:

Q: Which of the following is the example(s) of acid-base reaction? H H `H H -Br II IV OH H-CI OH

A: Acid- The species which is able to donate H+ ion.   Base-  The special which is able to accept H+…

Q: pH

A:

Q: Calculate 3OH-4 and pH for 2.250 g of LiOH in 250.0 mL of solution,

A: Molarity (M) It is the number of moles of solute dissolved in volume of solution in liters. M=number…

Q: HCN is a weak acid (Ka = 6.20 x 10-10), so the salt, KCN, acts as a weak base. What is the pH of a…

A: Given: Ka of HCN = 6.20×10-10 KCN = 0.0675 M we have to determine the pH ? Kb = Kw / Ka       = 1 ×…

Q: The Ka of propanoic acid (C,H,COOH) is 1.34 x 10-5. Calculate the pH of the solution and the…

A:

Q: a) What is the pH and pOH of 0.001 M NaOH solution, which is the strong base? b) The Ka value of…

A: pH + pOH = 14 pOH = -log [OH-] For a weak acid: [H+] = (Ka x C)1/2 Where, C = molar concentration

Q: What is the Ka of a weak acid whose 0.10 M solution produces a pH of 2.38?

A:

Q: If the Ka of a monoprotic weak acid is 8.3 × 10-6, what is the pH of a 0.19 M solution of this acid?

A: Given, Concentration of monoprotic weak acid = 0.19 M Ka of monoprotic weak acid = 8.3 × 10-6

Q: 5) What is the mass of Ca(OH)2 should be present in 0.250 L of solution to obtain a solution to…

A:

Q: For an aqueous solution of hydrochloric acid with pH = 0.500, what volume of 0.150 M sodium…

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Q: What is the pH of a 80.0 mL solution which is 0.27 M in IO and 0.49 M in HIO? The Ka for HIO is 2.3…

A:

Q: The Ka for niacin is 1.5 x 10-5. Whatis the pH of a 0.010 M solution of niacin?

A: The dissociation reaction of niacin is as shown below Hence we can see that 1 molar concentration…

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

A: given  HClO Ka=4.0 x 10-8  concentration of  NaClO IS 0.027  PH =?

Q: 04// (A) Calculate pH of 1.2 gm Sodium hydroxide in 200 ml distilled water?

A:

Q: What is the pH of a solution that is prepared by adding 30.23 mL of 1.77 M NaOH to 0.646 L of 0.476…

A: THIS WILL FORM AN ACIDIC BUFFER AS THE AMOUNT OF WEAK ACID(HN02)WILL REMAIN IN EXCESS AFTER REACTION…

Q: How many moles of NH3  would need to be added to 512.9 mL of a 0.25 M solution of NH4Cl to produce a…

A:

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: What is the theoretical pH of a 0.10 M NH4Cl solution when the Kb for NH3 is 1.8 x 10^-5?

A:

Q: What is the pH of 5.04 x 10-3 M HI? Is it acidic, basic, or neutral?

A: HI is a strongest acid it dissociates completely .

Q: 6. How many moles of benzoic acid (HC-HsO2) must be used to prepare 500. mL of a solution that has a…

A:

Q: What is the pH of a 1.0 x 10 M BalOH), solution at 25 °C: 7

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Q: The pH of a 0.060 M weak monoprotic acid, HA is 3.44. Calculate the Ka of the acid.

A:

Q: If 0.0751 moles of NaOH is added to 1.00 liters of 0.180 M CH3COOH (acetic acid), what will the pH…

A:

Q: What volume of 2.036 mol L-1 solution of LIOH is required to make 7.80 L of a solution with a pH =…

A: Given :-  Initial concentration of LiOH solution = 2.036 mol.L-1  pH of final solution = 12.80…

Q: 1.4 A 0.015 M solution of hydrogen cyanate , HOCN, has a pH of 2.67 a) What is the hydronium ion…

A: Given: The pH of the solution of hydrogen cyanate is 2.67. The molarity of hydrogen cyanate is 0.015…

Q: The pH of a 0.55 M aqueous solution of hypobromous acid, HBrO, at 25oC is 4.48. What is the value of…

A: The concentration of HBrO solution = 0.55 M. pH of aqueous HBrO solution = 4.48.

Q: What is the pH of a solution that is 0.32 M H(C6H5COO) and 0.12 M Na(C6H5COO)?   The Ka of…

A: Answer:- This question is answered by using the simple concept of calculation of pH of solution…

Q: pK, for the phenolate ion, C¿H;O¯, a weak base, is 4.204. Calculate the pH of a 0.339 M solution of…

A:

Q: Calculate the pH for 2.250 g of LIOH in 250.0 mL of solution.

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Q: A 1.00 L solution contains propanoic acid (C3 Hs O2 H) with a concentration of 0.210 mol/L, and…

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Q: If a buffer solution is 0.240 M in a weak acid (Ka = 3.8 x 10-5) and 0.530 M in its conjugate base,…

A: Introduction Henderson - Hasselbalch equation gets used to calculate the pH for any buffer solution…

Q: The Ka of a weak monoprotic acid is 1.13 x 10-5. What is the pH of a 0.0777 M solution of this acid?…

A:

Q: The pH of a solution at 25°C in which [OH-] = 3.7 x 10-5 M is: 4.43 3.70 4.78 8.6 D 9.57

A: Given OH- = 3.7 x 10-5

Q: Acetic acid (CH,COOH, Ka = 1.80 x 10-5) is a weak acid, so the salt sodium acetate (CH,COONA) acts…

A: In the given question we have to calculate the pH of 0.384 M sodium acetate. the given ka of acetic…

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

A: pH = 7 +12 (pka + log c)

Q: 20) What will be the pH (aq., 25 °C) of 250.0 mL of a solution of 0.545 M HCOOH and 0.628 M HCOOK,…

A:

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red. 

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.