A 0.0059 M solution of H2SO4 would have a pH of... (choose the best answer) * 3.8 .0118 O 1.9 0.0059

Q: would

A: [H+] = mass of HCl / [ molar mass of HCl • volume of HCl Solution ]  [H+] = 0.500g / ( 36.46gmol-1 •…

Q: A solution is created by dissolvong 0.907 moles of HCl into water, making 13.9 Liters of solution.…

A: GIVEN: Number of moles of HCl into water= 0.907 moles Volume of solution= 13.9 liters To Solve:  The…

Q: Calculate the pH of a solution that is 0.0729 M LiC2H3O2 at 25°C.

A: LiC2H3O2 ( Lithium acetate) is the salt of a weak acid and strong base.   LiC2H3O2 → CH3COO- +…

Q: An aqueous solution at 25 °C has a pH of 6.45. Calculate the pOH. Be sure your answer has the…

A: Solution At 25°C, water will ionize as follows: H2O(l) + H2O(l) <--> H3O+(aq) + OH-(aq) the…

Q: A 0.709 M solution of an acid HA has a pH of 1.45. What is its percent dissociation?

A: Given data :- Given acid = HA Concentration = 0.709 M pH = 1.45  -log [H +] = 1.45  [H+] = 10-1.45 =…

Q: An aqueous solution at 25 °C has a pH of 6.49. Calculate the pOH. Be sure your answer has the…

A: Answer:- This question is answered by using the simple concept of calculation of pOH using the…

Q: Which of the following solutions would be expected to have a pH of 7.00?

A:

Q: An unknown weak base with a concentration of 0.0910 M has a pH of 10.70. What is the Kb of this…

A:

Q: What is the pH of a 0.0556 M NH, (aq) solution at room temperature? The base ionization constant of…

A:

Q: Calculate the pH of each of the following strong acid solution 5.00 mL of 0.250 M HClO4 diluted to…

A: The process applicable for lowering the particular stock solution's concentration gets addressed as…

Q: The pH of a solution of household ammonia, a 0.950 M solution of NH3, is 11.612. Determine Kb for…

A: We know that, pH can be expressed as the negative logarithm of H+, i.e.            pH = - log[H+]…

Q: Calculate the pH of a solution that is made by dissolving 0.174 g of CSOH (M.M. 149.912 g/mol) in…

A: CsOH is a strong base. So, it will dissociate completely into ions. Now, pH can be calculated by…

Q: em101 The pH of a 0.0049 M solution of Ca(OH), is

A: Given that: molarity of Ca(OH)2 = 0.0049 M To find: pH of 0.0049 M Ca(OH)2 solution?

Q: H3O

A: solution that is 0.855% HNO3 by mass means : 0.855 g HNO3 is present in 100 g of solution. Mass of…

Q: What is the pH of 0.15325 M COCA COLA solution?

A: What is the pH of 0.15325 M COCA COLA solution?

Q: How many moles of NH3 must be dissolved in water to give 819.8 mL of solution with a pH of 10.97? K,…

A:

Q: Calculate the concentration of an aqueous solution of NaOH that has a pH of 11.56. Express your…

A: Given:: pH = 11.56 [NaOH] = ?

Q: Fill in blanks(): If the pH of a solution increases by 3, the acidity of the solution (    ) by a…

A:

Q: Find the pH of 0.22 M solution of LiOH. Round to the hundredths place.

A: LiOH is a strong ase which undergoes complete dissociation in aqueous medium giving Li+ and OH-…

Q: Calculate the pH of ... .. 0.320 moles of H,SO, dissolved in 8.0 L of water.

A: Given moles of H2SO4 = 0.320  Volume of water = 8 L

Q: What is the pH of a 0.00100M

A: Negative logarithm of H+ is called pH, to know the acidity of dilute solutions pH is introduced. pH…

Q: If the ?b of a weak base is 5.9×10−6,5.9×10−6, what is the pH of a 0.28 M 0.28 M solution of this…

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Q: What is the pH of a solution with a concentration of 0.00001 moles/ml (M) of H1?

A: Gvien, concentration of 0.00001 moles/ml (M) of H1

Q: Determine the pH of a solution that is 3.85% KOH by mass. Assume that the solution has density of…

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Q: The graph given below shows [H+] versus concentration foran aqueous solution of an unknown…

A: a) Since the concentration of H+ i.e [H+] is increasing with increase in the concentration of…

Q: o simplify the measurement of the acidity or basicity of a solution, the pH (hydrogen potential)…

A: Given[H+] = 0.0000375 pH = To be determined

Q: An unknown weak base with a concentration of 0.0910 M has a pH of 10.90. What is the Kb of this…

A:

Q: Calculate the pH of each of the following strong acid solutions: 5.00 mL of 0.250 M HClO4 diluted to…

A:

Q: What is the original molarity of an aqueous solution of ammonia (NH3 ) whose pH is 11.16 at 25°C? (…

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

Q: Determine the pH of an aqueous solution at 25.0 °C in which [H+] is 0.0025 M.

A: Given,     [H+] = 0.0025 M The pH of the solution is:

Q: A solution contains equal concentrations of an Acid and it's conjugate base. If the ka of the acid…

A: A mixture of a weak acid and its conjugate base (or a mixture of a weak base and its conjugate acid)…

Q: The pH of a solution is (6.5x10^0). What is the [OH-]? Report your answer to 2 sig figs. Note: Your…

A: Given, pH of the solution = 6.5 × 100 = 6.5 Concentration of the OH- ion = [OH-] = ? The formula…

Q: aqueous

A: Here, Kb value of Codeine is not given,  But the Kb value of Codeine weak base is 1.6 • 10^-6

Q: Calculate the pH of the following solutions.  1.50 g of NaOH in 50 mL of the aqueous solution

A: Given: The amount of sodium hydroxide present in 50 mL of water is 1.50 g.

Q: What is the pH of a 6.20 x 10-3 M NaOH solution?  (This solution is basic, concentration is of OH-)

A:

Q: Calculate the pH and pOH of an aqueous solution that is 0.75 % HCI, by mass, and has a density of…

A: Given :-  % by mass of HCl = 0.75%  density of solution = 1.04 g/mL  To calculate :-  pH and pOH for…

Q: An unknown weak base with a concentration of 0.170 M has a pH of 9.42. What is the Kb of this base?

A: Given is Concentration (c) = 0.170 M pH = 9.42 Kb = 0.170

Q: An unknown weak base with a concentration of 0.0910 M has a pH of 12.30. What is the Kb of this…

A:

Q: The pH for 1.0 × 10⁻³ M solution of cocaine, a weak base, is 9.70. Determine the value of Kb for…

A: Cocaine can be denoted as B. Concentration of OH- ions in cocaine can be determined as follows,

Q: An unknown weak base with a concentration of 0.170 M has a pH of 9.64. What is the Kb of this base?

A:

Q: For each strong acid solution, determine (H;O'], [OH¯], and pH. a. 0.25 M HCI b. 0.015 M HNO, c. a…

A:

Q: As much as 8 grams of NaOH (Mr = 40) is dissolved in water until the volume of the solution becomes…

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Q: The hydrogen ion concentration of a basic solution is 9.60 × 10-10 M. What is the pH of the…

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Q: Calculate the [H3O+] in solutions with the measured pH values shown here:A.pH = 7.35 B.pH = 3.45

A: Provided pH of solution (A)=7.35 Provided pH of solution (B)=3.45 Since, Concentration of H3O+=10-pH

Q: Express the pH of the solution ot three decimal places. 20.00 mL of 1.20 M HCl diluted to 0.570 L

A: Initial concentration, M1 = 1.20 M Initial volume, V1 = 20.00 mL Final volume, V2 = 0.570 L = 570 mL

Q: An unknown weak base with a concentration of 0.0910 M has a pH of 11.70. What is the Kb of this…

A: A weak base is a substance that do not dissociate completely.

Q: A solution is made by dissolving 27.5 g of HONH₃ClO₃ in 500.0 mL of water. Determine the pH of the…

A: Given: Mass of HONH₃ClO₃ = 27.5 g Volume of Water = 500.0 mL To Calculate: The pH of the solution

Q: Exactly 250 ml solution was made by dissolving 0.01 g of NaOH in water. What is the PH for the…

A:

Q: For a 0.0000125 M H2SO4 solution, the hydroxide concentration would be?

A: Answer = 3.98 x 10-10

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.