Which refers to a measure of how acidic or basic a solution is? O pH O solubility O reactiveness O hardness

Q: The molar concentration of OH- in a water solution is 1.0 x 10-9. The pH of the solution is

A: OH — = 1.0 x 10—9

Q: A student uses red litmus paper to test the pH value of different solutions. Which would result in a…

A: Explained as follows

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: HCIO4 is an example of: Select one: O Monoprotic Acid O Triprotic Acid O Diprotic Acid O Tetraprotic…

A: A monoprotic acid is the one which gives one proton when dissolved in water. A diprotic acid is the…

Q: All of the following are weak acids except O HCNO O HBr O HF O HNO, O HCN

A: An acid which dissociates completely or almost completely in water are strong acids.An acid that…

Q: Based on the following chemical reaction determine if H.CrrO is an acid or a base. determine if it…

A: 15. According Bronsted acid-base theory, Acid is the substance which gives H+ ions. Base is the…

Q: Calculate the pH of a solution that has a hydronium ion concentration, [H,O*], of 4.82 × 10-5 M. pH…

A:

Q: pH is O The measure of how acidic or basic a solution is The measure of how much water can attract…

A: PH is scale determine acidic and basic In nature.

Q: The [OH-] concentration of a solution is 6.78 x 10-6 M. The solution is O basic O acidic O neutral

A:

Q: The molar concentration of OH in a water solution is 1.0 ´ 10 -9. The pH of the solution is

A:

Q: Calculate the pH of each of the following solutions: a. [H3O+] = 2.0 x 10-12mol/L b. [OH-] = 4.5 x…

A:

Q: Determine the pH of a solution that has a hydrogen ion concentration [H+] equal to 3.2x10-5 mol/L.

A: In the question, The concentration of hydrogen ions present in a solution is provided. The pH of the…

Q: If a sample of calcium carbonate requires 22.50mL of 1.25M HCl to neutralize it, how many grams of…

A: The reaction taking place is  CaCO3 + 2 HCl -------> CaCl2 + H2O + CO2  hence from the above…

Q: A solution is made by dissolving 18.4 g HCI (MM=36 g/mol) in 662 mL of water. The pH of the solution…

A: HCl is strong acid

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 2.4×10-2 M. The hydronium ion…

A: By using hydronium ion and hydroxide ion concentration we can find pH and pOH of solution.

Q: For each of the following substances, predict the pH when each is dissolved in water.  Is it basic,…

A:

Q: Which of the following statements about different salts is TRUE? Select one: O a. An aqueous…

A: The statement about different salts which is True is given below.

Q: A solution has a hydrogen ion concentration of 1.43 x 10 M, Calculate the pH and select the…

A:

Q: what ion is responsible for basic properties in a water solution? a) potassium ion b) hydroxide ion…

A: hydroxide ion   Bases, on the other hand, all form a hydroxide ion, OH –( aq), in water. These…

Q: Calculate the pH of an aqueous solution of 0.2100 M potassium sulfite. pH =

A:

Q: A solution is made by dissolving 18.4 g HCI (MM=36 g/mol) in 662 mL of water. The pH of the solution…

A: given, mass of HCl = 18.4 g Molar mass of HCl = 36 g/mol Volume = 662 mL

Q: Write the equation that describes the equilibrium that exists when nitric acid dissolves in water.…

A: Acids on dissolving in water dissociates into ions. Hence Nitric acid will ionise into ions when…

Q: Which of the following is the weakest base? O fluoride anion, F2 O bromide anion, Br? O chloride…

A:

Q: [H*] [HO] pH Acidic, Basic, Neutral

A: at the 250C the product of H+ and OH- is always 1x 10-14 M pH < 7 = acidic pH > 7 = basic pH =…

Q: If the conjugate acid of a pair is chlorous acid, then what is the name of the conjugate base? O…

A: given that, chlorous acid is a conjugate acid.

Q: Calculate the pH of each solution and indicate whether the solution is acidic or basic.(a) [H3O+] =…

A: pH of the solution is calculated as, pH =-logH+

Q: Indicate the pH of the following

A: pH = -log[H+]  pH + OH = 14

Q: Which of the following is not identified as a weak acid? ο ΗΝΟ o H3PO4 o H2SO4 O HF

A: A strong acid has 100 % ionization while a weak acid has less percentage to 0% ionization.This…

Q: Which is an Arrhenius base ? O HCI Na OMBCI "OSHO

A:

Q: xplain the difference between pH value of distilled water and the theoretical pH expected

A: Distilled water is extremely purified water, but it also does not contain healthy minerals in it so…

Q: Which one of the following molecules is a strong acid? Select one: o Ca(OH), O HF O NH, HClo,

A:

Q: In water, a strong acid O is completely dissolved and completely ionized O is completely dissolved…

A: In this question, we will see the nature of strong acid in water.  You can see details explanation…

Q: Determine the pH of a solution

A: Given :-  Concentration of CH3COOH = 0.50 M  Concentration of CH3COONa = 0.30 M  To calculate :-  pH…

Q: which one of the Folow ing is NOT an exampie of an acidic acidl? o Sodium dinydrog en phosphate o…

A: If any compound have very low pH, then it's means the compound have higher acidic property,…

Q: Use the equation of the dissociation of the weak acid and a Le Schatelier principle to answer the…

A:

Q: How many mL of 0.45 M HCl(aq) are needed to neutralize a 149 mL solution of 1 M Ba(OH)2

A: Molarity is defined as number of moles of solute divide by volume of solution

Q: Which of the following is a strong acid? O acetic acid O hydrochloric acid Ohydrofluoric acid O…

A:

Q: A solution has a pH of 9.3. Is the solution O neutral O basic O acidic

A: pH determines the nature of a solution.  Solutions with pH less than 7 is acidic.  Solutions with pH…

Q: OH ACI Br OH Br Br CID ОН DIT Br. ОН ITY

A:

Q: Which one of the following 1.0 M solutions would be expected to have the highest pH? A) H₂SO4 B)…

A: We have to tell among the given 1.0 M solutions which one has the highest pH. The given solutions…

Q: 3. Describe how the pH of a solution would change if the solution becomes more acidic as HCl is…

A: The pH of a solution would change if the solution becomes more acidic as HCl is added to the…

Q: Calculate the concentration of OH2 ions in a 1.4 3 1023 M HCl solution Calculate the concentration…

A: The question is based on the concept of PH and pOH calculations.   pH is defined as negative…

Q: Which of the following is a weak acid? O H2SO4 O NH3 О Ba(ОН)2 Ο HI Ο ΗΝΟ,

A: We have to predict the weakest acid.

Q: Calculate the pH of each solution.

A:

Q: Calculate the pH and indicate whether each of the following solutions is acidic, basic or neutral…

A: If the pH is 1 to below 7, then it is acidic. If the pH is 7, then it is neutral. If pH is above 7…

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 3.2×10-² M. The hydronium ion…

A:

Q: What is an Arrhenius acid? Give an example?

A: An Arrhenius acid is a molecule which when dissolved in water will donate an H+ in solution

Q: A solution of 2.292 X 10-9 M HCl is __________. acidic basic neutral…

A:

Q: Which of the following will have the highest pH? O Lici О но НЗРО4 КОН

A: pH is a scale used to specify the acidity or basicity of an aqueous solution. Acidic solutions…

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.