I place 20.0 mL of deionized water and 2.0mL of 0.10 M NaOH in a beaker. What is the calculated pH?

Q: Phosphoric acid, H3PO4 is a triprotic acid.    pKa1= 2.16      pKa2=7.21            pKa3=12.32…

A: Given data, Molarity of HPO42-=0.450MpKa1=2.16pKa2=7.21pKa3=12.32

Q: Calculate the pH of water at 25°C and 75°C. The values for pKw at these temperatures are 13.99 and…

A: Pure water has an equal concentration of hydrogen ions and hydroxyl ions. The dissociation of water…

Q: The pH of a 1.00 × 10² M solution of cyanic acid (HOCN) is 2.77 at 25.0 °C. Calculate Ka for HOCN…

A: Solution :         The process of dissociation involves the segregation of molecules into smaller…

Q: Human sweat can have a pH ranging from 4.0 to 6.8. Calculate the range of [H3O+] in normal human…

A: Given, pH ranging from 4.0 to 6.8

Q: What is the pH of a 1.00x 10 molar solution of LICI? Report your answer with 2 places past the…

A: The acid-base nature of the salt solution depends on the nature of the acid and base from which the…

Q: Derive equations that define a0, a1, a2 and a3 for the triprotic acid H3X

A: In the titration of acid H3X, changes in the concentration of various species can be visualized from…

Q: 5. A solution is prepared by adding 1.00 x 1013 mole of strong base NaOH to 1.00 L of aqueous…

A: In this question we have to tell the pH of the given solution.

Q: Do you think the pH of 1.0 M tri-methyl ammonium (CH3)3NH", pKa 9.80, will be higher or lower than…

A:

Q: What is the pH of a solution prepared by dissolving 3.00 g of the weak acid HA (molar mass- 138.12…

A: pH of the solution indicates that the solution is acidic or basic in nature.  If the pH of the…

Q: Would a 1.0 * 10-8M solution of HCl have pH 6>7, pH = 7, or pH <7?

A:

Q: Calculate the pH of a solution prepared by dissolving 5.00 g of NaCIO in 400.0 mL of water.

A: Mass of NaClO  = 5.00g Volume of solution = 400.0 mL=400 ×10-3L Ka = 2.9 × 10-8

Q: Calculate the formate ion concentration and pH of a solution that is 0.050 M in formic acid (HCOOH,…

A:

Q: Consider the following data on some weak acids and weak bases: acid base Bo K, name formula name…

A: The given compounds are salts. So to check their pH , we would determine how these salts are made.…

Q: The concentration of OH- in a solution of householdbleach is 3.6 × 10-2 M. Calculate the pH of the…

A: Given here the Concentration of OH- in a solution [OH-] = 3.6 ×10-2 M . we are asked to calculate…

Q: The [H3O+] of lemon juice is 2.5 x 10-2 M.  Calculate the pH.

A: Given  [ H3O+ ]  = 2.5 × 10-2 M  PH = ?

Q: The pOH of ammonium hydroxide at 25 C is 5.55. What is the pH and the [H ], [OH ] in mol/L for…

A: At constant temperature, the pH of a solution remains constant. For 250 C, the pH of the solution…

Q: What is the pH of a solution of 5.94 M of HASO, which has K,= 5.1 x 10- Round and report your answer…

A: Concentration of H3AsO3 is 5.94 M. The value of acid dissociation constant is 5.1×10-10.

Q: What is the pH of the solution obtained when 130 mL of 0.610 M NaOH is diluted to 16.0 L with water?…

A: Given: Initial concentration of NaOH = 0.610 M Initial volume of solution = 130 mL = 0.130 L…

Q: What is the pH of a solution containing 9 gram of HCl (MW 18 am) dissolved in 50 ml of water?

A: In order to calculate the pH of solution we need to calculate firstly the number of moles of HCl.…

Q: You are given 30 Calculate the values of both pH and pOH of the following solutions: pOH pH 0.020M…

A:

Q: Define concept of Acid Strength and pKa ?

A: Acid strength means the tendency of acid to dissociate into H+ and anion. The dissociation of strong…

Q: The pH for 0.0715 M solution of CCl,CO2H is 1.40. Determine the value of Ka for CCl,CO2H. 1 2 Based…

A: pH of Solution = 1.40 [CCl3COO2H] = 0.0715 M Ka for CCl3COO2H =?

Q: What is the pH of a solution prepared by dissolving 0.748 g of Ca(OH)2 in water to make 517 mL of…

A: Given,

Q: Consider the following data on some weak acids and weak bases: acid base Ka K, name formula name…

A:

Q: Maleic acid (H2C4H2O4) is a diprotic acid with ?a1=1.20×10−3 and ?a2=5.37×10−7. Determine the pH of…

A: 1- First we will determine the H+ ion concentration :  Most H+ ion comes from first dissociation.…

Q: The pKw of seawater at 25°C is 13.776. This differs fromthe usual pKw of 14.00 at this temperature…

A: Given data contains, pKw of seawater is 13.776. pH in seawater is 8.00. Actual pKw of  water is…

Q: Ascorbic acid (vitamin C, C6H8O6) is a diprotic acid (Ka1 = 8.0×10–5 and Ka2 = 1.6×10–12). What is…

A:

Q: 1. Calculate the pH of a solution prepared by dissolving 2.13 g of picric acid, (NO2);C6H2OH (229.11…

A:

Q: The pH of a 0.05 M NaOH solution at 25 °C is: O 13.8 O 13.1 O 1.5 • 12.7 O 10.3

A:

Q: I place 20.0 mL of deionized water and 2.0 mL of 0.10 M HCl into a beaker. What is the calculated…

A: The total volume of solution present in the beaker is 22.0 mL.

Q: Ascorbic acid (vitamin C, C6H8O6) is a diprotic acid (Ka1 = 8.0×10–5 and Ka2 = 1.6×10–12). What is…

A: Solution -

Q: Ascorbic acid (vitamin C, C6H;O6) is a diprotic acid (Ka1 = 8.0x10 and Ka2 = 1.6×10-12). What is the…

A:

Q: Calculate the pOH and the pH of a 2.0×10−5 M solution of NaOH at 25°C

A: NaOH is a strong base. Hence it will dissociate completely as NaOH ------> Na+ + OH-  Hence…

Q: Ascorbic acid (vitamin C, C6H8O6) is a diprotic acid (Ka1 = 8.0×10–5 and Ka2 = 1.6×10–12). What is…

A: For first ionization :  pH = 0.5pKa1 - 0.5logC ..(1) Here, pKa1 = -logKa1 = -log(8*10^-5) = 4.097 C…

Q: How many moles of H₃O⁺ or OH⁻ must you add to 5.6 L of HA solution to adjust its pH from 4.52 to…

A: Strong acids and strong bases dissociate completely in their aqueous solution to provide H3O+ and…

Q: NH3 is a weak base (?b=1.8×10−5Kb=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the…

A:

Q: Why is the pH of water at 25oC equal to 7.00?

A:

Q: Consider the following data on some weak acids and weak bases: acid base Ka K, name formula name…

A: The compounds given are KCN, C6H5NH3Br, NaNO2 and KBr.

Q: How many grams of NaHCO3 must be added to 4 g K2CO3 to give a pH of 10.80 in 500 ml total solution?

A: Henderson-Hasselbach equation is given by: pH = pKa + logA-HAwhere [HA] is the concentration of the…

Q: 5. A solution is prepared by adding 1.00 x 1013 mole of strong base NaOH to 1.00 L of aqueous…

A: Here we are required to find the pH of NaOH solution

Q: Calculate the pH and pOH for the following: a. 10mg of cyanic acid (pKa=9.21) in 1L of water

A:

Q: The Kb of dimethylamine [(CH3)2NH] is 5.90x10–4 at 25°C. Calculate the pH of a 0.103 M  solution of…

A: Given : Concentration of (CH3)2NH = 0.103 M And Kb of (CH3)2NH = 5.90 X 10-4  Since (CH3)2NH is a…

Q: Calculate the formate ion concentration and pH of a solution that is 0.050 M in formic acid (НСООН,…

A:

Q: How many moles of (CH3)3N  would need to be added to 459.2 mL of a 0.25 M solution of (CH3)3NHCL  to…

A:

Q: Saliva has a pH range of 5.8–7.1. Approximately what is the H3O+ concentration range of saliva?

A: The concentration of the H3O+ ion present in a solution can be related to the pH of the solution as…

Q: What is the pH of a solution prepared by dissolving 8.13 grams of NaCN (49.01 g/mol) in 1.4 L of…

A: Given,  The pH of a solution prepared by dissolving 8.13 grams of NaCN (49.01 g/mol) in 1.4 L of…

Q: Caffeine (CHiON O2) is a weak base with a pKof 10.4. Calculate the pH of a solution containing a…

A:

Q: Determine the pH of a solution a) when 41.5 g of lactic acid is dissolved with water and diluted to…

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.