Question 52 (1 point) Formic acid, HCOOH, is a weak acid with a Ka equal to 1.8x104, What is the ph of a 0.0115 M aqueous formic acid solution?

Q: The pH of an orange juice is 3.33, calculate its [H+] and [OH-]

A: We can determine the hydronium and hydroxide ion concentration by applying the formula of pH =…

Q: A theoretical compound B3(OH)2 is a strong base that has a pH of 13.51. Determine the concentration…

A: The given data is as follows: The pH pf B3OH2 solution = 13.51 The concentration in molarity = ? The…

Q: Ignoring significant figures, what is the pH of a solution where [OH‒] = 1.0 x 10-9 M?

A: [OH-] = 1.0 x 10-9 M pH = ?

Q: Calculate the pH at 25 ° C of a 0.0033 M solution of a weak base with a Kb of 2.5 × 10−9 . pH =

A: Given:Kb = 2.5×10−9.Weak base [BOH] = 0.0033 M.

Q: It was determined that the pH of a sample of river water is 5.83. What is the H⁺ concentration of…

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

Q: What's the pH of the solution? See attached image. Please show steps.

A:

Q: What is the resulting pH of a solution that forms when 15.00 mL of a 0.150 mol/L hydrochloric acid…

A: Solution -  Given values  volume of  HCl= 15.00 mL  molarity of HCl= 0.150 mol/L  volume of sodium…

Q: Explain how the ion HC O 3 - can be both an acidand a base.

A: HCO3- is amphiprotic species because it can accept a proton as well as it can donate a proton.…

Q: Calculate the pH of the following solution 7.1 × 10−4 M Ba(OH)2:

A: Concentration of Ba(OH)2  is 7.1×10-4 M 1 mol Ba(OH)2  = 2 mol OH-,  So concentration of OH- is =…

Q: A solution that has a hydrogen ion concentration equal to 9.61 x 10-7 has a pH =

A:

Q: What is the pH of a 0.0250 M solution of HONH₃Cl (Kb of HONH₂ is 1.1 × 10⁻⁸)?

A: pH can be calculated as follows

Q: If pH is equal to 3.92, what are the values of H+, poH, and OH-?

A:

Q: Calculate the concentration of H30" in a solution of H,S04 that has a pH of 3.5.

A: Given: pH=3.5 To Find: [H3O+] =?

Q: Strong Bases; Calculate pH [base] [H3O"] pH Step 1 The strong base dissociates completely in aqueous…

A:

Q: What is [H] in a 0.450 M solution of acrylic acid, CH₂CHCOOH (Ka = 3.16 × 105)?

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Q: What is the pH of a 0.0550 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10-1⁰)?

A:

Q: pH

A:

Q: A diprotic acid (H₂A) has Kal = 4.12 × 10-7 and K₂2 = 5.14 x 10-¹¹. What is the pH of a 0.332 M H₂A…

A: A diprotic is the one which is capable of donating 2 H+ ions in aqueous solution .

Q: Calculate the hydronium ion concentrations of the following solutions at 25°C, given the pH. (a) pH…

A: Given :-  a) pH = 9.22  b) pH = 3.64  To calculate :-  Hydronium ion concentration i.e. [H3O+] in…

Q: "Acid rain" forms when rain falls through air polluted by oxides of sulfur and nitrogen, which…

A: 1) Here given---- pH of the acid rain = 3.41 We know---- pH = - log [H+] Or, [H+] = 10-pH  Now…

Q: If the (H*) in a solution is 6.23 x 10$ M. What is the pH?

A: PH is  defined as the power of Hydrogen.it measure acidity, basicity or neutrality of aqueous…

Q: calculate the {H3O} of the solution of hydrochloric acid with pH = 2.00

A: Given, PH = 2.00 PH is defined as negative logarithm of concentration of [H+] ions.

Q: 10) What is the pH of an Al(OH)3 solution with a concentration of 0.0182 M?

A:

Q: Caculate the pH of a solution in which [H3O+]= 1.5 x 10-3 M

A:

Q: a Calculate the pH of a solution that is 0.20 M HOCI and 0.92 M KOCI. Ką = 3.5x10-8 pH =

A: We will use buffer equation

Q: 6. Calculate the pH of the solution if the concentration of [H3O] ion is 2.0x10 M at 25°C.

A:

Q: Determine the pH of a 2.79 M solution of acetic acid (CH3COOH, ka=1.8x10-5)

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Q: What is the pH of a solution that has an OH- ion concentration of 3.20 M?

A:

Q: A solution has a pH of 3.4, what is [H*]? 2.51 x 10-11 M 3.4 M 3.98 x 10-4 M 07M

A: pH of a solution is defined as the negative logarithm of hydronium ion concentration.…

Q: Calculate the following for a 0.225 M solution of a weak acid with Ka=2.1×10^−8. [H3O+] =  pH =…

A: Ka of a weak acid(HA) = 2.110-8Molarity of HA = 0.225 MKw = 1.010-14

Q: Complete the balanced chemical reaction for the following weak base with a strong acid. In this…

A: In the given reaction between ammonia (NH3) and hydrochloric acid (HCl), ammonia is a weak base and…

Q: What is the pH of a 2.4 M solution of HC104? pH =

A: We have to calculate the pH of 2.4 M solution of HClO4.

Q: If the Kb of a weak base is 6.2 × 10-6, what is the pH of a 0.39 M solution of this base?

A: We know that; pH = -log (H+) And, pOH = -log (OH-) And ,pH + pOH =14

Q: Question 3 A student is given a concentrated solution that is supposed to contain vinegar, a weak…

A: A weak acid will not be completely dissociated in a solution. However, a strong acid will be…

Q: Determine the pH of a 0.33 M solution of NH4Br

A: Since we know that, Pkb(NH3) = 4.74.. Since NH4Br is salt of strong acid and weak base..

Q: 2-12 If 200 mg of HCI is added to water to achieve a final volume of 1.00 L, what is the final pH?

A:

Q: Calculate the pH of pure water if [H3O+] = 1.0 x 10-7.

A: PH is the power of Hydrogen. PH is used to determine nature of solution like as acidic,basic or…

Q: Carbonic acid, H,CO3 is a diprotic acid with Ka1 = 4.3 × 10-7 and Ka2 = 5.6 x 10-1". What is the pH…

A:

Q: What is the pH of a solution that has a [OH] = 3.3 x 10-³ M

A: pH is the negative logarithm of the concentration of H+. pOH is the negative logarithm of the…

Q: What is the pH of 0.0190 M NaOH?

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: The pH of a 0.0060 M solution of HNO₃ is

A:

Q: Calculate the pH of a sulfuric acid (H2SO4, Ka HSO4 = 1.2 x 10-2) solution that has a concentration…

A:

Q: What is the pH of a solution if [OH-]=2.4 x 10-6?

A: pH of any solution in terms of [OH-] is given by  pH = 14 + log[OH-] where [OH-] = concentration of…

Q: What is the pH of a 0.40 M solution of K₂SO3?

A:

Q: What is the pH of a solution with a hydrogen-ion concentration of 1 x 10-4 M?

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.