23 What is the pH of a solution composed of 0.20 M NH3 and 0.15 M NH.CI? (Kb NH3 = 1.8 x 10*)" (a) 2.15 (b) 4.62 (c) 8.26 (d) 9.38

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

A:

Q: What is the pH of a 0.660 M solution of NaCN (Ka of HCN is 4.9 × 10⁻¹⁰)?

A: The pH will be 11.56.

Q: Nitric acid (HNO3) is a strong acid that is completely ionized in aqueous solutions of…

A: Given:Concentration of HNO3 = 7.50 M% dissociation of HNO3 = 33%We need to calculate the Ka of HNO3

Q: t is the pH of a 0.4 rant chemical equar

A: Given: The concentration of the acid, (C) = 0.475 M. The Ka for the acid, (Ka) = 1.34 ×10-5.

Q: What is the pH of an aqueous solution composed of 0.64 M NH4+ and 0.20 M NH3? (Ka of NH4+ = 5.6 ×…

A: Given: Molarity of NH4+= 0.64 M Molarity of NH3= 0.20 M

Q: Calculate the pH and concentrations of CH3NH2 and CH3NH+3 in a 0.0341 M methylamine (CH3NH2)…

A: The given data contains, Concentration of methylamine = 0.0341 M. Kb of CH3NH2 is 4.47×10−4.

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: What is the pH and pOH of a solution if the molarity of the LIOH solution is 1 X 10 * M? -6

A: pHand pOH is defined for acid and base in generally. we will use formula to get the answers

Q: What is the pH of a 0.570 M solution of NaCN (Ka of HCN is 4.9 × 10-10)?

A: NaCN dissociates in an aqueous medium as follows: NaCN→Na++CN- Na+ ions don't contribute to the pH…

Q: b Answered Ata particular tempex Question 20 of 23 What is the pH of a 0.340 M solution of NaCN (Ka…

A: HCN in aqueous solution break as HCN= H++ CN- Now at equilibrium let concentration of H+= conc. of…

Q: Chemical pH #1 2 #2 9 #3 12 # 4 Which of the following chemicals will be a strong base? 1 3 4

A: Given  PH of different chemical = 2 ,9 ,12,5  Strong Base = ?

Q: 7-18. What is the pH of an aqueous solution that is 14.0% HCI by weight and has a density of 1.054…

A: Given information,      An aqueous solution that is 14.0% HCl by weight and has a density of 1.054…

Q: What is the pH of a 0.750 M solution of NaCN (Ka of HCN is 4.9 × 10-10)?

A:

Q: (d) Do you expect the pH of the pure water at 100 °C will be 7, lower than 7, or higher than 7? Give…

A:

Q: Calculate the pH of a 0.40 M CH3COOna solution. Kb for CH3COO- = 5.6*10^-10. (Show the dissociation…

A: First calculate the OH- ions concentration in the solution, and then pOH and then the pH of the…

Q: What is the pH of the hypothetical diprotic HydroRoseburgic acid with a concentration of o.75M? You…

A: Assume diprotic acid as H2A First dissociation of acid is         H2A (aq)+ H2O(l) -->HA-(aq) +…

Q: What is the pH of a solution that is 0.150 M NH3 and 0.200 M NH4CI? Kb of NH3 = 1.8 x 10-5 O9.26…

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Q: (Q7) If the initial concentration of the weak base ammonia in a solution is 0.401 M and the solution…

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Q: Milk of magnesia is often taken to reduce the discomfort associated with acid stomach or heartburn.…

A: When a base is added to  an acid, the acid gets neutralised. All the H+ ions present in the acid…

Q: b Calculate the pH of the following solution from the information given: РОН - 4.75 pH =

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

Q: 10

A: NaCN is a salt of strong base and weak acid. The pKa of HCN can be calculated as follows-

Q: What is the pH of a of 0.450 M NaCN? The Ka for hydrocyanic acid is 4.9 × 10-10?

A: Any certain salt solution achieves acidic or basic behavior when it undergoes hydrolysis reaction.…

Q: 3. If the solution with the pH of 2.30 had a concentration of 0.05 M, what is the percent ionized…

A: P.S.: According to the company guideline we have to answer the first question. So, please kindly…

Q: pH of 2.91 is prepared by dissolving I g. of benzoic ater. What is K of benzoic acid?

A: According to the question, a solution with a pH of 2.91 is prepared by dissolving 1 g. of benzoic…

Q: 1. 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: Note: As per the guidelines, solution of first question has been. For the expert solution of second…

Q: A weak base, B, has a concentration of 0.155 M. If the pH of the solution is 11.24, what is the K of…

A:

Q: Given that K, for water is 2.4 x 10 1 at 37 °C, calculate the pH of a neutral aqueous solution at 37…

A: Temperature plays a significant role on pH measurements. As the temperature rises, molecular…

Q: A 0.245−mol sample of HX is dissolved in enough H2O to form 595.0 mL of solution. If the pH of the…

A: pH= 3.60

Q: 2) The PH of asolution of aweak ronoprotic ucid (HA) is 2.85 what is the Ka of the acid ? Ans.: 2*10

A: Given ,  Concentration of weak mono protic acid ( C ) = 0.1 M pH of the weak acid = 2.85 Acid…

Q: The ionization constant for water (kw) is 2.9 × 10^-14 at 40 °C. Calculate [H3O], [OH], pH, and pOH…

A:

Q: Benzoic acid, C6H5COOH, is a weak acid (Ka = 6.28*10-5). If I dissolve 1.22 g of C6H5COOH in enough…

A: Molarity of benzoic acid (M)= No of moles / Volume in Liter No of moles = Mass / molar mass = 1.22 /…

Q: 3. What is the value of k"?

A: OH- + C24H30N3+  C23H30N3-OH The general rate law is   [rate] = k [OH-]^x [ C24H30N3+]^y For the…

Q: Determine the pH of a 0.461 M C6H5CO2H M solution if the Ka of C6H5CO2H is 6.5 x 10-5. RICE Table is…

A: RICE table is the initial, change and equilibrium concentration of chemical species taking part in a…

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: Which of the following statements is/are true? (Select all that apply) OThe higher the concentration…

A:

Q: An acid (HA) dissociates as follows: HA ? H+ + Aminus Arrow should be interpreted as an…

A: pH is the negative logarithm of concentration of proton. pH=-log[H+] It tells about the acidity of…

Q: 2. What is the value of k?

A: OH- + C24H30N3+  C23H30N3-OH The general rate law is   [rate] = k [OH-]^x [ C24H30N3+]^y For the…

Q: NH3 is a weak base (K, = 1.8 × 10-5) and so the salt NH¼C1 acts as a weak acid. What is the pH of a…

A: Given : concentration of NH4Cl = 0.088 M Since the salt given is a soluble ionic salt. Hence it will…

Q: The value of Ka for hydrofluoric acid is 7.20×10-4. What is the value of Kb, for its conjugate base,…

A: Kw = Ka × Kb  Ka is the acid dissociation constant whereas Kb is the base dissociation constant.  Kb…

Q: The pH of a solution is 6. What is the pOH? pOH = %3D What is the hydrogen concentration? [H*] = Is…

A: The pH of a solution is used to determine the alkalinity or acidity of a solution. The pH of a…

Q: What is the expected pH of a 150.0 mL 0.250 M solution of HOCI which is diluted to a 500.0 ml mark…

A: Given that, a 150.0 mL of 0.250 M solution of HOCl is diluted to 500.0 mL, i.e., V1 = 150.0 mL, S1 =…

Q: What is the pH of a 0.870 M solution of Ca(NO2)2 (Ka of HNO2 is 4.5 × 10*)?

A: dissociation of Ca(NO2)2 Ca(NO2)2(aq)→Ca2+(aq)+2NO2-(aq) we can see 2mol of NO2- is formed from 1…

Q: Whats pH of a solution that is 0.010 M in HClO Ka = 3.5 × 10–8 and 0.010 M in HCl?

A: Since HCl is a strong acid, it is completely dissociated into H+(aq) and Cl-(aq).  Hence [H+(aq)] =…

Q: What is the concentration of hydroxide ion in a 0.170 M aqueous solution of hydroxylamine, NH2OH?…

A: pH of solution is defined as negative logarithm of hydrogen ions concentration.

Q: calculate the ionization constant of the acid. 5. What concentration of NH3 is required to make a…

A:

Q: The artificial sweetener saccharin (shown below) is a weak acid (pKa = 2.32 at 25 °C). It is used in…

A: Given that, pK of Saccharin = 2.32 Also, pK = -logKa Ka = 10-2.32 = 4.8 x 10-3 Also, Kw=Ka.Kb…

Q: A weak base has a Kb of 4.29E-10. Calculate the pH of a 0.250M solution of the weak base.

A:

Q: Calculate the pH and concentrations of CH3NH2 and CH3NH+3 in a 0.0395 M methylamine (CH3NH2)…

A: CH3NH2 is a weak base.  Hence, pOH = 0.5pKb-0.5logC ..(1) pKb = -logKb = -log(4.47*10^-4) = 3.35…

Q: presence of an acid, su

A: Organic reactions are those in which organic reactant react to form organic products.

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.