4. Suppose you had a sample of Hydrobromic acid that had a molarity of 0.1 and you had 42 ml of it. If you added 20 ml of 0.15 M NAOH, what is the pH of the resulting solution? NaOH + HBr -> NaBr H2O

Q: Calculate the pH for basic solution pOH =6?

A: The relation between pH and pOH is  pH +pOH = 14 Given pOH = 6

Q: Determine the pH of an aqueous solution that is 0.078 M in HCIO4 and 0.080 M in HNO3. O 1.5 O 0.98 O…

A: By using the formula of pH and by calculating total H+ concentration we can calculate pH.

Q: Determine the concentration of H+H+ ions in an aqueous solution where [OH−]=1.45×10−4…

A: Given: [OH−]=1.45×10-4 M [H+] =?

Q: Which could be the pH level for a solution of sodium hydroxide? о в. 7.0 О с. 11.2 O D. 2.3

A:

Q: What is the pH of a solution containing 3.2 x 10-6 M hydronium ions

A: The pH of a solution determines the acidity and basicity of a solution, which is calculated using…

Q: What is the pOH of a 0.030 M Sr(OH)2 solution? a. 12.78 b. 12.48 O C. 1.52 O d. 1.22

A:

Q: Write the balanced NET IONIC equation for the reaction that occurs when hydrobromic acid and…

A: An acid is a substance that gives H+ ions in its solution whereas a basic substance gives OH- ions…

Q: n chemistry, the pH of a solution is a measure of the acidity or alkalinity of a solution. Water has…

A: Given : Concentration of hydrogen ion = 8 x10-8 M.

Q: Calculate the pH of a 0.600M solution of tin chloride SnCl2.

A:

Q: 5. Calculate the pH and pOH for each of the following solutions at 25°C. a. 1.0 x 10-3M OH - b. 1.0…

A:

Q: Question attached

A: There are two types of bases/acids. One is strong base/acid which is completely dissociable in into…

Q: The OH ion concentration of a blood sample is 2.6 x 10 M. What is the pH of the blood? blood O a.…

A: pH  =  - log [ H3O+ ]  pOH  =  - log [ OH- ]  pH  +  pOH   = 14

Q: Calculate the pH and pOH of: 0.3M sulfuric acid (H2SO4) solution

A: Given:  Molarity of H2SO4=0.3M

Q: Determine the pH of an aqueous solution that is 0.078 M in HCIO, and 0.080 M in HNO3. O 2.1 O 0.98 O…

A: concentration of HClO4=0.078M Concentration of HNO3=0.080M pH of aqueous solution=?

Q: A solution of hydrobromic acid has [HBr] = 1.3×10-2 M. What is the pH of this solution

A: As per guidelines if multiple questions, first question is allowed to answer, please post  questions…

Q: 8) What is the pH of a 0.035 M HNO, solution? HNO; (aq) + H,O (1) H3O* (aq) + NO3 (aq)

A:

Q: Consider the ncutralization reaction 2 HNO, (aq) + Ba(OH), (aq) 2H,O(1) + Ba(NO,),(aq) / A 0.115 L…

A: Ans: Balanced equation  2HNO3 (aq) + Ba(OH)2(aq)→2H2O (l) + Ba(NO3)2(aq) Molarity of…

Q: Write a balanced chemical equation to represent each of the following acid-base neutralization…

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

Q: a) Calculate the molarity of AlCl3 if 0.220 mol AlCl3 is dissolved in enough water to make 0.500 L…

A: The moles of AlCl3 is = 0.220 mole The volume of solution is = 0.500 L The molarity of the solution…

Q: The pH of a solution of HBr was 2.633. What was the hydronium ion concentration?

A: pH =  - log(H+)

Q: Aqueous permanganate ion may also be reduced using aqueous bromide ion, Br−, the products of this…

A: The oxidation (O) and reduction (R) half reactions taking place are  O: Br- → BrO3-          =>…

Q: What is the pH of a 0.0338 M nitric acid, HNO3, solution?

A:

Q: Calculate the pH and the pOH of a solution containing a H3O+ concentration =2.5 x10^-2M.

A: p H can be calculated using the equation given below:

Q: A sample of calcium hydroxide (Ca(OH)2) has a concentration of 0.00473 mol/L. What is the pH of this…

A: The PH of Ca(OH)2 can be calculated as follows

Q: Determine the concentration of oxygen ions in 0.5000 M SnO3

A: Given  Concentration of SnO3  = 0.5000 M  Concentration of oxygen ion = ?

Q: What is the pH of an aqueous solution with a hydronium ion concentration of 1.75 × 10⁻⁵ M?

A: We know that, pH is the negative logarithm of hydronium ion concentration. i.e.,…

Q: What is the hydronium ion concentration for a 0.265 M solution of HCIO that has a K, -2.9 x 10? What…

A:

Q: 1 You are presented with a solution that has a pOH of 2.13,What is the pH of this solution? O 11.87…

A: The pOH of the solution is = 2.13 The pH of the solution is =?

Q: For  K w, the product of [H 3O +] and [OH -] is

A: Kw is the water constant and is defined as product of hydronium ion and hydroxyl ion  Kw = [H3O+]…

Q: What are the products of the reaction between barium hydroxide Ba(OH)2 and hydrogen chloride (HCI)?…

A:

Q: pOH

A:

Q: The reaction of magnesium hydride (M9H2) with water (H2O) is an acid-base reaction. What is the acid…

A:

Q: What is the pH of a 0.031 M solution of aqueous Sr(OH)2? 1.21 1.51 12.49 12.79

A: pH :-  The negative logarithm to the base 10 of hydrogen ion concentration expressed in mol/L of a…

Q: 9.) The pH of an HCl solution is 3.0. a.) What is the pOH of this solution? b.) What is the H3O+…

A:

Q: The following reaction is in equilibrium: NO2 (aq) + H20 (1) = HN02 (aq) + OH" (aq). Kh (NO,) = 2.2…

A: According to Le Chatelier's principle, when a system at equilibrium is disturbed, then the system…

Q: What is the concentration of hydroxide ions with a pH of 4.76?

A: Given : pH = 4.76

Q: What is the pH of a 0.031 M solution of aqueous Sr(OH)2? O 1.21 O 1.51 O 12.49 O 12.79

A: pH of an aqueous solution is defined as the negative logarithm of H3O+ ion concentration.…

Q: Write the balanced NET IONIC equation for the reaction that occurs when hydrochloric acid and…

A: It is given that Hydrochloric acid (HCl) is reacting with ammonia (NH3) and the net-ionic equation…

Q: what is the ph of a 0.81 M hypochlorous acid (HClO) solution?

A: Given :- concentration of HClO = 0.81 M                 Ka = 3.0 × 10-8  To calculate :- pH of…

Q: Pd(PPh,), `B(OH)2 KOr-Bu Br. H,0

A: This is an example of intramolecular Suzuki coupling reaction.

Q: 10.0 ml of 1.15 M chlorous acid is added to 1.00 L. of water. Determine the new concentration of…

A: From data  M = 1.15 M  V of acid = 10.0 mL = 0.01 L  V of water = 1 L  Formula used Molarity =…

Q: If a 1.5 L sodium hydroxide solution contains 38g of NaOH, what is the pH of the solution?

A: We have to calculate the pH of Solution.

Q: Br NaOH МеCN

A: The given reaction is take place by SN2 mechanism.

Q: According to the Arrhenius concept, if Al(OH)3 were dissolved in water, it would act as: A) a…

A:

Q: How many moles of hydroxide ions can be released into solution from 1.00 mg of Mg(OH)2 that is used…

A: Molar mass of Mg(OH)2 = 58.32 g/mol Given mass = 1 mg = 0.001g Moles = 0.001/58.32 = 1.71*10-5

Q: Consider the neutralization reaction that occurs between sulfuric acid and sodium hydroxide. How…

A: Buffer solution is defined as the aqueous solution which consists of a weak base/acid and its…

Q: Write a balanced chemical equation for the following reaction in a basic solution. ClO–(aq) +…

A: Write a balanced chemical equation for the following reaction in a basic solution.ClO–(aq) +…

Q: Molecules of different acids ionize to form different numbers of ions. Both HCl and HNO3 are…

A:

Q: If HCI is added to each of the following substances, which will produce CO2 gas? KBr СаСОз NaOH…

A: Answer  If HCl is added to each of the following substance…

Q: AgH KCN HBRO, 4(aq)

A: Since you have posted a question with multiple sub-parts, we will solve the first three subparts for…

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.