Assuming complete dissociation, what is the pH of a 4.57 mg/L4.57 mg/L Ba(OH)2Ba(OH)2 solutio

Q: weak monoprotic acid (HA) has an acid ionization constant Ka = 1.8x10° at 298 K. If 100 mL of a 0.10…

A: First write equilibrium equation for reaction of weak acid and strong base and fine limiting…

Q: Calculate the pH of a solution that was prepared by mixing 25.00 mL of a 0.1630 M HClO4 solution…

A: pH is a parameter which is used to determined the acidity or basicity of an aqueous solution.  pH is…

Q: Use the drop down menu to answer if these statements about the polyprotic acid are true or false.…

A: We have to tell whether given statement are true or false

Q: Which statement is False?  I     A 0.100 M solution of LiOH will have a pOH that is less than 7.…

A: 1) since LiOH is a base and will produce OH- ions in solution  hence the pH of base will be > 7…

Q: Calculate the pH of a solution when 10.00 mL of 0.1000 M NaOH is added to 20.00 mL of 0.1000 M…

A: Given: Concentration of CH3COOH = 0.100 M Volume of CH3COOH solution = 20.00 mL = 0.020 L…

Q: You are asked to estimate the pH of a 15mL of 0.09 N of HCl when 16.9mL of 0.085 N NaOH is added to…

A: Here 15 ml of 0.09 N HCl is added to 16.9 ml of 0.085 M NaOH solution. After that 100 ml of diluent…

Q: 6. Calculate the pH of each of the following solutions: a. 2.8x10-4 M Ba(OH)2 b. 5.2x10-4 M HNO3

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: What is the pH of a solution that is 0.400 M in NH3 and 1.450 M NH4*? Ka= 5.7x1010

A: Given :-  Concentration of NH3 = 0.400 M  Concentration of NH4+ = 1.450 M  Ka = 5.7 × 10-10  To…

Q: The benzoate ion, C6H5COO-, is a weak base withKb = 1.6 x 10-10. How many moles of sodium benzoate…

A:

Q: Determine the pH of each two-component solution. a. 0.050 M KOH and 0.015 M Ba(OH)2b. 0.265 M NH4NO3…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: Propionic acid, HC3H5O2, has Ka= 1.34 x 10–5. (a) What is the molar concentration of H3O+ in 0.15 M…

A: HC3H5O2 is a weak acid and dissociates in aqueous solution as: HC3H5O2+H2O↔C3H5O2-+H3O+

Q: Which of the following is the pH of the solution containing 0.01 mol CH3COOH and 0.820 grams of…

A: Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…

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: What will be the pH of 0.025 M NaOH solution in H2O at 60 °C? (KW60°C = 1.0 x 10-11) A. 1.6 B. 9.4…

A:

Q: please highlight the correct answer

A: Given, [H3O+] = 3.25*10-2

Q: What is the pH of a solution prepared by mixing 100.00 mL of 0.020 M Sr(OH)2 with 50.00 mL of 0.400…

A: Strontium hydroxide and lithium hydroxides are strong bases. They dissociate completely in the…

Q: Which solution has the higher pH, a 0.001 MM solution of NaOHNaOH or a a) 0.001 MM solution of…

A: Calculate the pH of 0.001 M solution of NaOH: NaOH completely dissociated to form one Na+ and one…

Q: 1) Calculate percent concentration of a 150-gram solution containing 30 g Salt. 2) Calculate…

A: Formula used:  1) Percent concentration of a solution=( mass of solute/mass of solution) × 100 2)…

Q: If you are titrating a 20.0 mL of a 0.100 M solution of  HCl with 0.100 M NaOH, what is the pH of…

A:

Q: What is the pH of a 0.1000M Ca(OH)2 solution? 9.50 13.30 11.50 12.30 0.70

A: Given: Molarity of Ca(OH)2 solution = 0.1000 M

Q: 27. What is the pH of a 0.42 M solution of sodium propionate, NAC3H5O2, at 25°C? Ko(C3H5O2 ) = 7.69…

A: M

Q: 5.02

A: This question is related to pH.

Q: used as preservatives in vinegar, soy sauce, etc. The pH of a 0.10 M aqueous solution of sodium…

A: Sodium benzoate is salt of weak acid-strong base type salt pH = 1/2(14 + pKa + log([C]) 8.60 =…

Q: What is the pH of a 0.300 M NH 3 solution that has Kb = 1.8 x 10 ? The equation for the dissociation…

A: The pH of solution can be calculated as follows

Q: A concentrated hydrochloric acid solution contains 36.0% HCl (density = 1.18 g/mL). How many liters…

A:

Q: What is the pH of a cleaning solution with a  [H30+]= 7.4 × 10^9M  [H3O+]

A: To calculate the pH of a cleaning solution to following calculation is used

Q: 3. If you had 36 ml of a .14M solution HBr that you mixed with 40 ml of a .11M solution of RBOH,…

A:

Q: What is the pH of a 8.4 x 10–5 M Ba(OH)2 solution?

A:

Q: Calculate the pH of a solution that is 0.54 M HF and 1.00 M KF. Ka = 7.2x104 pH =

A: Given, Concentration of HF = 0.54 M Concentration of KF = 1.00 M Ka for HF = 7.2 x 10-4  PH = ?

Q: 8. The normal pH of human blood ranges from 7.35 to 7.45. Calculate the concentrations of H3O* and…

A: Given,  pH  = 7.45 [H3O+] = 10-pH = 10-7.45 = 3.55×10-8 M   [OH-] = 10-14/[H3O+]  = 2.82 × 10-7 M

Q: What is the pH of a 0.015 M Ba(OH)2 solution? Ba(OH)2  is a strong base.

A:

Q: A 1.24 L solution contains 0.010 M HCN. What volume of 0.0086 M NaOH must be added to achieve a pH…

A: First the reaction between acid and base is noted. Now use Henderson-Hasselbalch equation,

Q: 6. Which of the following has the highest pH? a. 1.00 M NaNO3 b. 1.00 M NaNO2 c. 1.00 M NaH,PO4 d.…

A:

Q: A solution of HCNO (Ka = 3.5 x 10“) has a pH of 2.3. What is the concentration of this solution?

A: After observing this question, we can say that, This question is completely based on "Handerson -…

Q: Calculate the pH of a solution when the following quantities of .7500 M KOH are added to 60.00 ml of…

A: Hello. Since the question consists of multiple sub-parts, the first three sub-parts will be solved.…

Q: The pH of a Ba(OH) 2 solution is 10.00. What is

A: pH is equal to the negative logarithm of hydrogen ions

Q: Find the pH of a solution prepared by dissolving 12.43 g tris (121.136) plus mol' 4.67 g tris HCI…

A: Given: Mass of tris = 12.43 g Mass of tris HCl = 4.67 g Molar mass of tris = 121.136 g/mol Mass mass…

Q: What

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid

Q: 4. The concentration of H* ions in a bottle of table wine was 3.2 x 10-24 M right after the cork was…

A: Given data: Initial concentration of H+ ion is H+=3.2×10-24M  Final concentration of H+ ion is…

Q: If the Ka of a monoprotic weak acid is 1.4×10−6, what is the pH of a 0.14 M solution of this acid?

A: Given information: Concentration of an acid = 0.14 M Ka of weak acid = 1.4×10-6

Q: A buffer solution is prepared by dissolving  1.700 g of ammonium chloride (NH4Cl) into 100.00 mL of…

A: Mass of ammonium chloride is 1.7 g. Molar mass of ammonium chloride is 53.491 g/mol.

Q: what is the pH of a blood sample with a molar mass concentration of H+ ions as 7.2x 10^-8

A:

Q: 4. If you had 98 ml of a .60M solution of HCN that you mixed with 110 ml of a 0.50M solution of KOH,…

A:

Q: If there is a solution of weak acid (CH3COOH) and a solution of strong acid (HCl), what statement is…

A: Strong acid dissociates completely in water to give H+ and conjugate base whereas weak acid do not…

Q: A 0.10 M aqueous solution of which of the following salts will have the lowest pH? A. Ni(NO3)2 B.…

A: Since the solution should be having lowest pH. Hence the solution will be most acidic because lower…

Q: The pH of a Ba(OH)2 (strong base) solution is 10. What is the H+ ion concentration of this

A: Given , PH  = 10  H+ = ?

Q: Assuming complete dissociation, what is the pH of a 3.22 mg/L3.22 mg/L Ba(OH)2Ba(OH)2 solution?

A: Consider the 1 L of solution. Then mass of barium hydroxide = 3.22 mg Lets find the concentration of…

Q: 1. A solution of Ba(OH)2 has a [OH-] of 0.40 M. What is the initial molar concentration of the…

A: Given,  [OH-] = 0.40 M  Substance = Ba(OH)2  What is the initial molar concentration of the solution…

Q: What is the pH of the solution resulting from mixing 187 mL of a 1.570 M solution of HBr with 116 mL…

A:

Q: The volume of an adult's stomach ranges from 50.0mL when empty to 1.0OL when full. a. If the volume…

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.