2. Calculate the pH of each solution: (a) 0.0155 M HBr (b) 1.28 × 10-3 M KOH (c) 1.89 × 10-³ M HNO3 (d) 1.54 × 10 4M Sr(OH)2

Q: What is the pH of a 0.660 M solution of NaCN (Ka of HCN is 4.9 × 10⁻¹⁰)?

A: The pH will be 11.56.

Q: The base Ca(OH)2 is almost insoluble in water , only 0,25 g can be dissolved in 0,5 L of water at 25…

A: Base is the substance which gives hydroxide ion in the solution while acid gives proton in the…

Q: If 8.5 grams of solid NaC2H3O2 (MW = 82.03 g/mol) are added to 100.0 mL of water, how many mL of 1.0…

A: Answer:- Henderson-Hasselbach equation :- This equation is used for the determination of pH or pOH…

Q: The ?a of a weak monoprotic acid is2.72×10−5. What is the pH of a 0.0751 M solution of this acid?

A:

Q: What is the pH of the solution obtained by mixing 35.00 mL of 0.250 M HCI and 35.00 mL of 0.125 M…

A:

Q: A solution is prepared by adding NaOH to pure water until a pH = 9.34 is obtained. Calculate the pH…

A:

Q: A 0.285−mol sample of HX is dissolved in enough H2O to form 605.0 mL of solution. If the pH of the…

A: Dissociation extent for any species is clearly visible in its dissociation constant value. If this…

Q: If the ?aKa of a monoprotic weak acid is 7.9×10−6,7.9×10−6, what is the pH of a 0.25 M0.25 M…

A: The question is based on the concept of equilibrium. we have been given a weak acid whose…

Q: If the ?bKb of a weak base is 1.5×10−6,1.5×10−6, what is the pH of a 0.34 M0.34 M solution of this…

A:

Q: A 0.020 M aqueous solution of a weak monoprotic base, B, has pH of 11.44. Calculate the value of Kb…

A: First write  Basic  medium reaction  B + H2O = BH+ + OH-

Q: A 4.9 × 10−3−mol sample of HY is dissolved in enough H2O to form 0.090 L of solution. If the pH of…

A: given, number of moles of HY = 4.9 × 10−3 Volume of solution = 0.090 L the pH of the solution = 2.55

Q: To increase the pH of 1.50 L of 0.25 M HCIO3 (aq), which of the following would you add to the…

A:

Q: If 8.5 grams of solid NaC2H3O2 (MW = 82.03 g/mol) are added to 100.0 mL of water, how many mL of 1.0…

A: GIVEN: Mass of NaC2H3O2=8.5 gVolume of NaC2H3O2=100 ml To solve: ml of 1.0M HCl needed to prepare a…

Q: a) The average pH of normal arterial blood is 7.40 at 37° C. Calculate [H] for blood at this…

A: a) Given : pH of blood = 7.40

Q: c) What mass of NaC₂H,O,₂ must be dissolved in 0.300 L of 0.25 M HC₂H₂O₂ to produce a solution with…

A: mass of NaC2H3O2 ,sodium acetate = ? Volume of NaC2H3O2 = 0.300 L [HC2H3O2 ] = [CH3COOH] = 0.25 M pH…

Q: A 75.00-mL portion of a solution that is 0.0460 M in HClO4 is treated with 150.00 mL of 0.0230 M…

A: Acid reacts with base to form salt and water. The given acid is HClO4 and base is KOH.

Q: Suppose that a benzoic acid (C,H,COOH) solution has a pH of 3.15. Which of these substances would…

A: Given substances: KCl C6H5COONa NaI HBr We have to find the substance that would increase the pH…

Q: A solution NaOH has 0,04%w/v. Find the pH of the solution, when it is given that the solution NaOH…

A: pH is defined as the negative logarithm of Hydrogen ion concentration. In Chemistry, pH denotes as…

Q: 2. The pH of a 0.100 M weak acid solution is 4.07. Calculate the K, value for the weak acid.

A: Hey, since there are multiple questions posted, we will answer first question. If you want any…

Q: What is the pH of a 0.730 M solution of NaCN (Ka of HCN is 4.9 × 10⁻¹⁰)?

A: Interpretation: The pH of a 0.730 M solution of NaCN is to be determined. Ka of HCN = 4.9 × 10-10

Q: Calculate 3OH-4 and pH for 2.250 g of LiOH in 250.0 mL of solution,

A: Molarity (M) It is the number of moles of solute dissolved in volume of solution in liters. M=number…

Q: If

A: Given: 50 mL of 2.00HCN(Ka=6.210×10-10) is diluted to 1.00 L. To find: pH of the solution.

Q: Suppose 0.0013 mol HA and 0.0013 mol A¯ are present in 170. mL solution and the pH is 4.00. What is…

A: Given: Moles of HA = 0.0013 mol. Moles of A- = 0.0013 mol. And the pH of the solution = 4.00

Q: 3. A solution is 0.0500 M in NH,Cl and 0.0300 M in NH3. Calculate its OH concentration and its pH.

A: Solution - pH =  pH, historically denoting "potential of hydrogen" is a scale used to specify the…

Q: What is the pH of a solution prepared by diluting 25.00mL of 0.020 M Ba(OH)2 with enough water to…

A: Ba(OH)2 is a strong base. It dissociates completely to give Ba2+ and OH- ions.  Ba(OH)2→ Ba2+ + 2OH-…

Q: 4. Calculate the pH of a solution that is 0.0532 M in acetic acid and 0.0245 M in sodium acetate.

A: Given-> Concentration of acetic acid = 0.0532 M Concentration of sodium acetate = 0.0245 M

Q: When 35.0 mL of 0.300 M hydrobromic acid and 35.0 mL of 0.300 M ammonia are combined, the pH of the…

A: Given molarity of HCI = 0.300 M Volume 35.0 mL = 0.035 L So, Number of moles of HC| = Molarity of…

Q: How many moles of NH3  would need to be added to 512.9 mL of a 0.25 M solution of NH4Cl to produce a…

A:

Q: 2.30 mL ofa 0.4375 M HCl solution are added to 35 mL of 0.250 NAOH solution. What is the final pH?

A: An acid HCl and base NaOH undergo neutralization reaction to form salt NaCl and water. For the given…

Q: If the ?a of a monoprotic weak acid is 7.5×10−6, what is the pH of a 0.30 M solution of this acid?

A: Given: The Ka of a monoprotic weak acid = 7.5×10−6 We have to calculate the pH of a 0.30 M solution…

Q: The pH of a 0.060 M weak monoprotic acid, HA is 3.44. Calculate the Ka of the acid.

A:

Q: Calculate the pH of the resulting solution when 35.00 mL of 1.000 M KOH is mixed with 65.00 mL of…

A: Given :  Molarity of KOH solution = 1.000 M Volume of KOH solution = 35.00 mL  Molarity of HCl…

Q: What will be the pH of the solution when 12.0 mL of 0.400 M KOH is added to a 25 mL of 0.200 M HOCI…

A: Given-> Volume of KOH = 12.0 ml Molarity of KOH = 0.400 M Volume of HOCl = 25 ml Molarity of HOCl…

Q: The pH of 750 mL (3 SF) of an aqueous solution containing only NaNO 2 is 8.42. If HNO 2 has a Ka of…

A:

Q: Which of the following acids is the best to prepare a buffered solution with a pH = 3.50? Justify…

A: A buffer solution is the mixture of a weak acid and its conjugate base in such a way so that…

Q: 3. Calculate the pH of the following solution that is a) 0.0100 M in HCl and 0.0200 M in picric…

A:

Q: The uses of sodium phosphate include clarifying crudesugar, manufacturing paper, removing boiler…

A: Na3PO4 + 3H2O --------> 3NaOH + H3PO4  Molecular weight if Na3PO4 = 163.94 g/mol  Molecular…

Q: Consider a 0.155 M LiCNO solution where Ka of HCNO = 2.0 × 10** Blocks a) Write the dissociation…

A: The question is based on the concept of  salt hydrolysis. the given salt is the salt of weak acid…

Q: What is the pH of a 0.870 M solution of Ca(NO2)2 (Ka of HNO2 is 4.5 × 10*)?

A: dissociation of Ca(NO2)2 Ca(NO2)2(aq)→Ca2+(aq)+2NO2-(aq) we can see 2mol of NO2- is formed from 1…

Q: Consider a solution which is 0.20 M in CH,COOH and 0.10 M in CH,COONA. Which of the following…

A: Option (e) is true.

Q: Calculate the pH for 2.250 g of LIOH in 250.0 mL of solution.

A:

Q: A CHM 122 student combines 42.2 mL of 0.413 MHBR with 32.7 mL of 0.384 M KOH. What is the pH of the…

A:

Q: What is the pH of a solution prepared by adding 0.253g of ammonium chloride to 0.241ml of water? Kb…

A: The Bronsted-Lowry acid-base theory was purposed by Bronsted and Lowery is called Bronsted-Lowry…

Q: 6. Label the following salts as acidic, basic or neutral. a) FeCl, b) KBr c) LICIO, d) NH,NO, e)…

A:

Q: III. Suppose you are given 500.0 mL of 0.25 M HOB1 and 500.0 mL of 0.25 M HBRO3. a. Draw a Lewis…

A: Acidity is decided on the basis of pKa value i.e. how easily an acid gives its proton in solution…

Q: What is the pH of a solution obtained by mixing 0.59 L of 0.100 M  Ba(OH)2 and 0.10 L of 0.118 M…

A: Acid and base are the chemical compounds which upon adding in water change the pH value accordingly.…

Q: What is the pH of the resulting solution if 25.0 mL of 1.12 M HCl is mixed with 60.0 mL of 0.25 M…

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.