For nitrous acid, HNO2, Ka = 4.0 × 10–4. Calculate the pH of 0.33 M HNO2.     A)  2.92   B)  1.94   C)  3.40   D)  0.48   E)  4.36

Q: Calculate the pH of the solution.  Assume 1.0 L of solution. You must identify the type of solution…

A: The salt of a strong base and weak acid are basic in nature and the pH of these salts is higher than…

Q: A chemist dissolves 108. mg of pure perchloric acid in enough water to make up 210. mL of solution.…

A: The given data is as follows: The mass of perchloric acid = 108 mg = 108×10-3 g=0.108 g The volume…

Q: Carbonic acid, H,CO, is a diprotic acid with Ka1 = 4.3 × 107 and Ka2 = 5.6 × 1011. What is the pH of…

A: H2CO3 ⇌HCO3−  +   H+.........     ka1= 4.3x10-7 HCO3− ⇌CO3-2 ​+   H+..........    Ka2=5.6x10-11ka1…

Q: What is the pH of a 0.360 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹

A: Given data--> C= 0.360 M solution of C5H5NHBr Kb=1.7*10-9   pkb = - log10(1.7*10-9) pkb= 9 -…

Q: Calculate the pH of a 0.170 M solution of potassium nitrite, KNO₂. pH =

A: Given that, [KNO2] = 0.170 M =C (LET)  pH = ?

Q: 6. Determine the pH and [OH] of a solution if its [H*] = 7.5 x 103M.

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

Q: b)Determine if the following solutions are acidic, neutral, or basic at 35 °C. Explain your answer.…

A: NOTE : In case of neutral water, H+ ions concentration is given has to be assumed as nothing is…

Q: Find the pH of a 2.0 M solution of H2SO4. Ka = 1.1 x 10^-2

A: Given :-  Concentration of H2SO4 solution = 2.0 M  Ka of H2SO4 = 1.1 × 10-2  To find :-  pH of…

Q: What is the pH of a 0.24 M solution of sodium propionate, NaC3H5O2, (base) at 25°C? (For propionic…

A:

Q: 1. Ca(OH)2 solution has a concentration of 9.66 x 104 M. Determine the pH of the solution.

A: From the Calcium hydroxide concentration, hydroxide concentration can be calculated.…

Q: Calculate the pH of water at 60 °C. The pKa of water is 13.017 at this temperature.

A: Since pKa = -log(Ka) => Ka = 10-pKa  = 10-13.017 = 9.62 X 10-14 approx H2O (l) -----> H+(aq) +…

Q: Determine the voltage of a galvanic cell composed of Pb(s) in a 1.00 M solution of Pb²+, and Ni(s)…

A:

Q: Consider an aqueous solution that is 0.050 M in H2Se (Ka = 1.29 x 104) and 0.075 M in NaHSe. Out of…

A: The acid ionization constant for acid is 1.29×10 -4.

Q: Determine the pH of a 0.650 M solution of magnesium nitrite, Mg(NO2)2 at 25 °C. A solution…

A: Answer: Hydrolysis of the salt of weak acid and strong base or strong acid and weak base takes place…

Q: Find the pH of 4.2 X 103 M HClO4.

A: pH can be expressed as the negative logarithm of H+ ion, i.e.                            pH =…

Q: What is the pH of a 0.250 M  solution of H2SO4? Ka2 = 1.20×10–2

A:

Q: . Calculate the pH of a 0.0368 M aqueous solution of nitrous acid (HNO2, Ka = 4.5×10-4).

A: HNO2 is a weak acid and does not undergo complete dissociation in solution.

Q: What is the pH of a 0.420 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)

A: Given, Concentration of C₅H₅NHBr = 0.420 M Kb = C₅H₅N is 1.7 × 10⁻⁹

Q: Stomach acids (HCL) has a pH of about 1.5. For individuals who suffer from acid refulx, antacids or…

A: We have to predict the balance chemical reaction.

Q: Find the pH of a 0.2 M solution of H2SO3

A: Given,  The pH of a 0.2 M solution of H2SO3 is:

Q: Calculate the pH of the following acid in water knowing that its concentration is 0.73 M and its Ka…

A: Step 1: To answer this question, we must use the ICE table. Initial, [HA] = 0.73 M ICE table:…

Q: HCl is a strong acid.  What is the pH of a solution of concentration 1 x 10-3M?

A:

Q: Calculate the pH of a solution that is made by dissolving 5.54 g NH4NO3 in enough water to create…

A: First to calculate morality Then to calculate degree of dissociation.  Then to calculate pH.

Q: Phosphoric acid, H, PO,(aq), is a triprotic acid, meaning that pKal pKa2 pKa3 one molecule of the…

A:

Q: Find the pH of a 0.043 M HClO4 solution.

A: Given :- concentration of HClO4 = 0.043 M  To calculate :- pH of the solution

Q: Percent ionization for a weak acid (HA) is determined by the following formula: [HA] ionized [HA]…

A: we have to calculate the percent ionization

Q: Which of the following solutions would have the lowest pH? Assume that they are all 0.10 M in acid…

A:

Q: 1) The pH of coffee is 4.9. What is the concentration of OH in coffee?

A: As per the company guidelines, we are authorised to solve only one question at a time. Please post…

Q: 7. a) Calculate the pH of a 2.0 M aqueous solution of H2SO4. b) Calculate the pH of a 5.0 × 10 M…

A: 7. a) calculating the pH of a 2.0 M aqua solution of H2SO4: Given;

Q: What is the pH of a 0.430 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

A: pH= 1/2(pKb-logc) Here given Kb=1.7×10-9,hence pKb=-logKb=-log(1.7×10-9) given c=0.430 M

Q: Hydrazine, N₂H4, is used as a rocket fuel, but also as a reactant in organic chemistry. The K, of…

A: moles of Hydrazine = 4.75 × 10-3 molVolume of the solution = 0.500 LKb of Hydrazine = 9.1 × 10-7pH…

Q: A solution has a pH of 3.76. What is the molarity concentration of H3O+ and OH¹ in this solution? A)…

A: The objective of this question is to determine the molarity concentration of H3O+ and OH- in a…

Q: Consider a solution initially containing 0.30 M of CH3NH2 mixed with 0.50 M of CH3NH3Cl in water.…

A:

Q: 5. a. Determine the hydrogen ion concentration, [H*] for a solution with a pH of 3.42. Is this…

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 0.270 M  solution of H2SO4? Ka2 = 1.20×10–2

A: Here given, Ka2 = 1.20 × 10-2 Concentration of  H2SO4 = 0.270 M

Q: Be sure to answer all parts. Enter your answer in scientific notation. Thiamine hydrochloride…

A: break down the solution step-by-step:**Step 1: Calculate the pKa value**The pKa value is a measure…

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.