13.3) Determine [OH–], pOH and pH of a 0.18 M  aqueous solution of LiC3H5O3 (K b = 7.1×10-11).

Q: Methylamine, CH3NH2, is one of several substances that give herring brine its pungent odor.  In…

A:

Q: What is the concentration of a solution of (a) KOH for whichthe pH is 11.89, (b) Ca(OH)2 for which…

A: We know that, the pH of the solution is equal to the negative log10 of the hydrogen ion…

Q: What is the pH of a 0.178 M aqueous solution of sodium cyanide, NaCN at 25 "C7 (K, for HCN= 4.0-10

A: The given information is: Concentration of sodium cyanide = 0.178 M Ka for HCN = 4.0 x 10-10 The…

Q: Determine the Ka of a 0.10-M solution of hydrogen sulfate ion, HSO₄⁻, that is 1% ionized.

A: Ionisation of Hydrogen sulfate.

Q: What is the pH of a 0.790 M solution of NaCN (Ka of HCN is 4.9 10-10)?

A: Given, Molarity of NaCN = 0.790M

Q: Phenylacetic acid (C6H5CH2COOH, simplified here to HPAc; see model) builds up in the blood of…

A: Solution- Given data: The pH of Phenylacetic acid = 2.62. The concentration of C6H5CH2COOH…

Q: What is the pH of a solution of 0.300 M HNO, containing 0.180 M NANO,? (Ka of HNO2 is 4.5 x 10-4)

A: Given- Concentration of HNO2=0.300M Concentration of NaNO2=0.180M Ka of HNO2= 4.5×10-4

Q: What is the pH of a 0.750 M solution of C,H,NHB (Kb of C,H̟N is 1.7 10°)?

A:

Q: Calculate the values of 3H+4 and 3OH- 4 in a neutral aqueous solution at 25 °C

A: SOLUTION: Step 1: A neutral solution indicates pH is 7. At 25 0C, the concentrations of H+ and OH-…

Q: The concentration of SO42- ion in a 0.25M Al2(SO4)3 solution is:

A: Given information: Concentration of aluminum sulfate = 0.25 M

Q: What is the percent ionization of a 0.75 M solution of ammonia? Kb(NH,) = 1.8 × 10-5 [?] %

A: Given ,  Ammonia concentration = 0.75 M Kb=1.8×10-5

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

A: Kw = Ka x Kb  Kw = 1x10-14  given that Ka = 4x10-8 find Kb = (1x10-14) / (4x10-8) = 2.5x10-7 Initial…

Q: What is the concentration of a solution of (a) KOH for which the pH is 11.89, (b) Ca(OH)2 for which…

A: We use the PH equation for calculation for H+ concentration.  Then apply Ionic  product  of water to…

Q: The benzoate ion, C6H5COO-, is a weak base with Kb = 1.6 * 10-10. How many moles of sodium benzoate…

A:

Q: The value of K, for nitrous acid is 4.50×10-4. What is the value of Kp, for its conjugate base,…

A: Given: Ka value of HNO2 = 4.50 ×10 ^-4 To find : Kb value of conjugate Base. Solution : As we know…

Q: What are the concentrations of each of the following species in 0.100 M Ascorbic acid: H2C6H6O6,…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: The hydroxide ion concentration, [OH-], of an aqueous solution of 0.421 M diethylamine (a weak base…

A: When the rate of forward reaction is equal to the rate of backward reaction then the reaction is…

Q: Which of the following statements is/are TRUE regarding a 0.20 M solution of the strong acid, HX? 1.…

A: Here we are required to find the statement true about strong acid.

Q: What volume of 0.252 M potassium hydroxide solution is required to completely neutralize 0.0106…

A: An acid base reaction is also called as neutralization reaction. The H+ ions of acid react with OH-…

Q: What is the pH of a 0.580 M solution of NaCN (Ka of HCN is 4.9 x 1010)?

A:

Q: The value of K, for benzoic acid is 6.30×10-5. What is the value ofKg, for its conjugate base,…

A: Given: For Benzoic acid  The value of Ka = 6.30 x 10-5  For Conjugate base, C6H5COO- The value of Kb…

Q: In an aqueous solution at 25 C, if [H3O+]=3.1×10^-4M, then [OH-] is

A: Given data: The hydronium ion concentration is H3O+=3.1×10-4 M. To find: The hydroxide ion…

Q: What is the percent ionization in a 0.300 M solution of formic acid (HCOOH) (Ka = 1.78 × 10-4)?

A:

Q: What is the pH of 0.0100mol.dm3 solution of a weak.,monoprotic acid K3=3.4×10-3 at 25°C?

A: Given concentration(C) = 0.0100mol/dm3 Dissociation constant ( K ) = 3.4×10-3

Q: Many moderately large organic molecules containing basicnitrogen atoms are not very soluble in water…

A: An acidic substance is the substance that can give H+ ions. They are corrosive and sour in nature.…

Q: Calculate the concentration (molarity) of HC2H3O2 in a solution that is 0.191 M LIC2H3O2 at 25°C.…

A: Given solution is lithium salt of acetic acid , so we can use its dissociation equation to calculate…

Q: At 25 °C, what is the hydroxide ion concentration, [OH−], in an aqueous solution with a hydrogen ion…

A:

Q: What is the percent ionization in a 0.590 M solution of formic acid (HCOOH) (Ka = 1.78 × 10⁻⁴)?

A: Since HCOOH is a weak acid. Hence it will dissociate partially in solution as HCOOH ----> H+ +…

Q: A solution is found to have a pH of 8.3, what is the hrdroxide ion [OH-] concentration?

A: Introduction If we know the pH of any particular solution, then first [H+] is calculated then with…

Q: if the concentration of hydrogen ionsis 6.33 x10''-3 what is the concentration of hydroxide ions?

A: concentration of hydrogen ion = H+ = 6.33 x 10-3 concentration of hydroxide ion = OH- = ?

Q: A 1dm3 aqueous solution contains 6.78g of barium hydroxide, Ba(OH)2.  What is the pH of the solution…

A: A numerical problem based on pH calculation, which is to be accomplished.

Q: Aspirin has the structural formula   At body temperature (37 °C), Ka for aspirin equals3 x10-5. If…

A:

Q: 16.110 Arrange the following 0.10 M solutions in order of increas- ing acidity: (i) NH,NO3, (ii)…

A: The salt hydrolysis can be explained as the reaction in which the acidic solution is generated if…

Q: Determine the (a) degree of ionization and (b) percent ionization of ethylamine, C2H5NH2 in an 0.85…

A: Given concentration of ethylamine = 0.85 M Standard value Kb for ethylamine = 4.3*10-4

Q: What mass (in g) of potassium fluoride should be added to 0.50 Lof 0.255-M HF(aq) at 25 °C to give a…

A: Given: Concentration of HF = 0.255 M Volume of solution = 0.50 L pH of buffer solution = 3.85  And…

Q: Sodium stearate (C₁₇H₃₅COONa) is a major component of bar soap. The Kₐ of the stearic acid is…

A: The pH of 10.0 mL of a solution containing 0.42 g of sodium stearate has to be given, Given, The Kₐ…

Q: At 25 °C, what is the hydroxide ion concentration, [OH–], in an aqueous solution with a hydrogen ion…

A: The formula for ionic product of water  is given.

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

A: Weak acid are those acid which does not dissociate completely in aqueous solution and weak base are…

Q: The pH of a solution at 25C 11 which OH =20x 10 is: 4.76 3.30 9.52 9.30 4.69

A: Concentration of OH- ion = 2.0 × 10-5  pH of the solution at 25°C = ?

Q: The Ka for formic acid (HCO2H) is 1.8x10-4, What is the pH of a 0.20M aqueous solution of sodium…

A:

Q: dissociated H+H+ ions

A:

Q: What is the pH of a solution that is 0.071 M LiCN at 25°C?

A: A solution is made up of 0.071 M LiCN at 25 ◦ C. Here, we have to calculate the pH of the solution.…

Q: At 25 °C, what is the hydroxide ion concentration, [OH−], in an aqueous solution with a hydrogen ion…

A:

Q: Q6) 200 ml , o.0ol M NAOH is udded to 30oml, o.0005 M HCL. what is the PH of the Soluution ? Ans. :…

A: The balanced Chemical Reaction between HCl and NaOH is - HCl + NaOH ----> NaCl + H2O Here, one…

Q: What is the percent ionization in a 0.270 M solution of formic acid (HCOOH) (Ka = 1.78 × 10⁻⁴)?

A:

Q: What is the PH of a l.6M Soluten of Ascorble Acid, th C HG OG Kaz -5 = 8.0 x10, Ke=1.6A 10-12)

A: Given: Concentration of H2C6H6O6 = 1.6 M Ka1 of H2C6H6O6 = 8.0 × 10-5 And Ka2 of H2C6H6O6 = 1.6 ×…

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.