9 Write the formula of the conjugate acid of a HSO, b CO;?

Q: What is the pH of a .100M CH3COOH(aq) solution?

A: Acetic acid is a weak acid, it does not dissociate completely but exists in equilibrium with acetate…

Q: . Strychnine, C,H„N‚O, (aq) is a weak base but powerfully toxic. (a) Calculate the pH of 0.001 mol/L…

A: Given: Concentration of weak base (assuming B) = 0.001 M And Kb of base = 1.0 × 10-6

Q: What is the pH of a 0.350 M solution of HF (Ka = 6.8 × 10⁻⁴)?

A:

Q: What is the pH of [H30+]= 2.4 * 10 3 M?

A: Given :- [H3O+] = 2.4 x 10-3 M  To calculate :- pH of solution   pH = -log[H3O+]

Q: What is the pH of a 0.590 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

A:

Q: What is the pH of a 0.100 M solution of LiBrO(aq) at 25'C? Assume that LiBrO is a strong…

A: Since you have posted multiple questions, we are entitled to answer the first only. Given:…

Q: Calculate the pH of a solution of ammonium acctate. Given that: K, - 1.76 x 10, K,- 1.8 x 10 and K,…

A: A salt formed of weak acid and strong base is alkaline in nature and has a pH above 7 while a salt…

Q: What is the pH of a 0.0500 M solution of HONH₃Cl (Kb of HONH₂ is 1.1 × 10⁻⁸)?

A: HONH3Cl is a salt and in solution it gets dissociated as HONH3Cl → HONH3+ + Cl- The hydrolysis…

Q: What is the pH of a 0.720 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

A:

Q: culate the pH of an 3.09 x 103 mol/L solution of hydrochloric acid to two wer:

A:

Q: 7. The pH of a 0.10 M solution of acetic acid (CH3COOH) is 2.39. What is the Ka of acetic acid?

A: H3O+ can be calculated as follows: pH=-log [H3O]+[H3O]+=10-pH[H3O]+=10-2.39[H3O]+=0.00407 M

Q: What is the pH of a 0.650 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

A:

Q: Arrange the following in order of INCREASING acidity. I. II. III. IV. ... ÇI CI HO HO HO HO

A: Given question of mainly phenol group.    We have difine a increasing acidic order.    Attached a…

Q: What is the pH of a 0.540 M solution of Ca(NO,), (Ka of HNO, is 4.5 x 10*)?

A:

Q: What is the pH of a 0.390 M solution of HF (Ka = 6.8 × 10⁻⁴)?

A:

Q: 2. The pH of a lime is 1.90. What is the [H3O*]?

A: pH is negative log of Proton concentration.

Q: What is the pH of a 0.320 M solution of Ca(NO,), (Ka of HNO, is 4.5 × 104)?

A: For HNO2 , pKa = -logKa                           = -log (4.5 x 10-4 )                           =…

Q: Using data from Appendix D, calculate 3OH-4 and pH for each of the following solutions: (a) 0.10 M…

A:

Q: Find the pH of a 0.22 M AlCl3 (aq) solution if Ka of Al3+ is 1.2 × 10–5

A:

Q: Calculate the pH of a 3.97×10³ M solution of NaF, given that the Ka of HF = 6.80 x 10-4 at 25°C.

A:

Q: Calculate the pH of a 0.75 mol L─3 solution of ethanoic acid at 298 K. Given Ka = 1.7 × 10─5

A: Welcome to bartleby ! We have to calculate pH .

Q: What is the pH of a 0.870 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

A: Answer:- This question is answered by using the simple concept of hydrolysis of the salt formed by…

Q: The pH of a lime is 1.90. What is the [H3O+]? What is the [-OH]?

A: Since the relationship between pH and  [H3O+] is  pH = -log[H3O+] and the relationship between pH…

Q: What is the pH of a 0.510 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

A: Given information: Concentration of solution = 0.510 M

Q: 1. Calculate pH and concentrations of the ions for ammonia aqueous solution with concentration 0.010…

A: Given that : The concentration of ammonia = 0.010 M The pKb of ammonia is 4.76. We have to calculate…

Q: C D B

A: Bronsted-Lowry Acid is any species that can donate a proton. When an acid and base react with each…

Q: Calculate the molar concentration of OH- in a 0.724 M solutionof hypobromite ion (BrO-; Kb = 4.0 x…

A: Since the BrO- will get hydrolysed by water as per the reaction => BrO- (aq) + H2O (l)…

Q: Which of the following substances can be classified as a Lewis base? CO Cu F a) O, only b) O, and CO…

A:

Q: What is the pH of a solution that has a [H3O+] = 4.5 × 10^_5?

A: Given:[H3O+] = 4.5 × 10-5 M.

Q: is acidic or cor [H*]

A:

Q: What is the pH of a 0.380 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

A:

Q: The concentration of H* (or H3O*) from part A should be 1.02×10¬2 mol L-1. What is the pH of the…

A:

Q: Calculate the pH of a of 0.100M KBRO solution. Ka for hypobromous acid, HBRO, is 2.0 x 10 6- 10.85…

A: Given: The concentration of the KBrO3 solution = 0.100 M The Ka for HBrO3 = 2.0 × 10-9 We have to…

Q: B. Calculate the PH and to YOH FOR 9.209 M Solution Cr (₂(04),

A:

Q: The molecule lactic acid (HC3H5O3) IS CONSIDERED A BRONSTED-LOWRY ACID. Write a chemical equation…

A: According to Bronsted-Lowry concept, an acid is a substance that can donate a proton i.e. H+ to the…

Q: What is the conjugate acid of potassium hydrogen phosphate, K2HPO4?

A: K2HPO4 is a base. Its conjugate acid can be obtained by adding a hydrogen atom to it. The net ionic…

Q: What is the pH of a 0.460 M solution of HF (Ka = 6.8 × 10⁻⁴)?

A:

Q: .Calculate the concentration of H3O+ in the sample of milk of magnesia with the pH=10.52 2.…

A: “Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: Give the formula of the conjugate acide of H2O ?

A: Conjugate acid, according to Bronsted-Lowry-acid-base theory, is chemical compound that is formed…

Q: A 0.539 M solution of oxalic acid (pK, = 1.23) is prepared. Determine the pH of the !3! solution.…

A:

Q: In the following reaction, identify the Lewis acid. Co** (ag) + 6NH3 (ag) - Co(NH3),**(aq)

A: Lewis acid is an electron-pair acceptor. That is Lewis acid is any substance which can accept a pair…

Q: A patient’s sputum was collected for a laboratory analysis. The results revealed that the [H3O+]…

A: Given data contains, The concentration of hydronium ion is 5.2 x 10-7 M.

Q: What is the pH of a 0.350 M solution of lithium citrate?

A: Lithium citrate is a salt of LiOH ( strong base ) and citric acid ( weak organic acid ). In case of…

Q: Calculate the pH of a solution of 0.25M Nacio(ag). The Ka of HCIO is 2.9 x 108.

A: NaClO is a salt of weak acid HClO. It has pH greater than 7 as it is base.

Q: Identify the conjugate acid of SO 4 2–.

A: In this question we have tell the conjugate acid of the given SO42-

Q: Which of the following is the stronger Brønsted–Lowry acid, HClO3 or HClO2?

A: Any chemical species able to gain (receive) a proton (H+) ion from another species gets referred as…

Q: Rank the following in order of increasing acid strength: HIO₃, HI, CH₃COOH, HF.

A: Given, HIO₃, HI, CH₃COOH, HF.

Q: The conjugate acid of H2O is

A: Conjugate acid is a chemical species same as original species combined with H+ ion.  In general, 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.