Research on the PH of these common household liquids. Solution pH pOH [H30*] [OH] Juice-lemon, 4 orange Vinegar Table salt 2.5 7 dissolved in water Soap solution Baking soda solution 10 8.3 Drain cleaner 14 Dishwashing 7 liquid eyewash 7.4

Q: What is the pH of a 0.375 M aqueous solution of methylammonium chloride? Kb (CH3NH₂) = 4.2 × 10-4…

A:

Q: What is the hydronium ion concentration of a solution with a pOH of 8.30?  1.28 × 10−6 M  1.99 ×…

A:

Q: What is the pH of a 0.40 M ammonia solution? Kb = 1.85 × 10-5

A: Ammonia = 0.40 M Kb =  1.85 × 10-5 Ammonia is weak base . Kb is the dissociation constant of Ammonia…

Q: 11.) Calculate the pH of the following solutions: a.) 0.100 M solution of HNO2 (Ka = 4.5 x 10–4)…

A: (11a)

Q: What is the pH of [OH−] = 2.4 × 10−9 ?  B   a. 2.4   b. 5.4 c. 8.6 d. 9.0

A: Given that -  Hydroxide ion concentration, [OH-] = 2.4×10-9  Then , Hydrogen ion concentration and…

Q: HC3H5O3, is found in sour milk. What is the pH of 0.30M lactic acid? Ka=1.4 ' 10-4

A: The reaction of lactic acid releasing H+ ion in water is given as-…

Q: Calculate the pH of a 0.700 M CH3NH3Cl solution. Kb for methylamine, CH3NH2, is 4.4 × 10-4. I need…

A: Hydrolysis of the salt is defined as the process of producing acidity or basicity to the solution…

Q: What is the [OH⁻] in an oven-cleaning solution if the pH is 12.35? A) 0.45 M B) 1.65 M C) 0.022 M D)…

A:

Q: A certain acid, HA, has a Ka given by: HA + H2O H3O* +A- Ka = 6.80 × 10-6 What is the pH of a 0.247…

A: Answer is explained below.

Q: The pH of a 0.244 M solution of sodium methanoate, HCOO-Na+, is 8.57. Calculate Kb for the…

A:

Q: What is the pH of a 0.025 M aqueous solution of Sr(OH) 2?   a. 12.40   b. 1.60   c. 1.30   d.…

A: The concentration of Sr(OH)2 = 0.025 M Strontium hydroxide is a strong base dissociates completely…

Q: What is the pH of the solution that is prepared when 121 g piperidinium chloride salt is dissolved…

A: Given: The amount of piperidinium chloride salt dissolved in 100 mL of water is 121 g. The volume of…

Q: Calculate the pH of a 0.512 M solution of a triprotic weak acid, H3A, given the acid ionization…

A:

Q: The pH of a 0.12 M HNO3 solution is -1.22 -0.92 0.92 1.22

A: Given concentration of HNO3 = 0.12 M

Q: What is the pH of 0.024M acetic acid solution at 25°C? (Ka=1.8×10^-5)

A: Given, [CH3COOH] = 0.024 M Ka = 1.8 × 10-5

Q: What is [H30+] in a solution of 0.25 M CH3CO2H and 0.030 M NaCH3CO2? CH3CO,H(aq) + H20(1) = H30*(aq)…

A: Acetic acid and sodium acetate form buffer solution

Q: What is the PH of a 0.13 solution of the salt NaX? Ka of HX= 1.5×10^-5

A:

Q: What is the pH of a 0.010 M solution of aqueous Sr(OH)2?   a. 10.2   b. 2.0   c. 9.0   d.…

A: To determine the pH of a basic solution, the pOH is determined first and then pH is calculated using…

Q: What is the pH of a 0.23 M solution of ammonium bromide? The Kb value for ammonia is 1.8*10-5.

A:

Q: 18) What is the pH of a 0.240 M solution of potassium cyanide? Ka (HCN) = 6.2 × 10-10 A) 4.9 B) 9.1…

A: GIVEN: Ka(HCN) = 6.2 *10-10 Concentration of KCN =0.240 M To Calculate: pH of the solution=?

Q: What is the pH of a 0.012 M Ca(OH), solution? 1.92 12.08 1.62 12.38

A:

Q: 5.796

A: Kb = 10-pKb  Kb = 10-5.796 Kb = 1.6 • 10^-6

Q: 3. What is the pH of 0.03 M acid solution? The Ka of the acid is 5x10-3? A. 1.5 В. 1.9 С. 2.0 D. 2.3

A: We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…

Q: What is the pH of the solution that is prepared when 121 g piperidinium chloride salt is dissolved…

A: Piperidiniun chloride : BH+ The reaction of Piperidiniun chloride with NaOH is given below. BH+ +…

Q: What is the pH of a 0.0013 M solution of niacin? Ka = 1.5x10^-5

A:

Q: What is the pH of the solution that is prepared when 121 g piperidinium chloride salt is dissolved…

A: Answer - The correct option is (d) 9.2 Solution -

Q: The pain reliever codeine is a weak base with a Kb equal to 1.6×10–6. What is the pH of a 0.250 M…

A:

Q: What is the pH of the solution that is prepared when 121 g piperidinium chloride salt is dissolved…

A: Given,  Mass of piperidinium chloride = 121 g  Volume of NaOH = 200 mL  Molarity of NaOH = 0.10 M…

Q: Phosphoric acid (H3PO4) is a weak acid naturally found in the body that supports kidney function and…

A: Given,    Phosphoric acid (H3PO4) is a weak acid and it's Ka value is 6.9 * 10-3 at STP…

Q: 0.215 M solution of acetate has a pH of 9.00. What is the Kb of acetate?

A:

Q: What is the pH of a 0.0600 M solution of nitric acid at 25 C? A) -1.22 B) 1.22 C) 0.06 D) 7.00 E)…

A: To find pH of nitric acid:

Q: What is the pOH of 0.003 M acetic acid solution (Ka = 1.8x10 5)

A:

Q: What is the pH of a 0.20M solution of nitrous acid? Ka= 4.5x10^-4.

A:

Q: What is the ph of a solution with (H3O)= 6.4 x 10- 7th power

A: The concentration of hydronium ion is provided, i.e. [H3O+]=6.4 x 10-7 pH of the solution=?

Q: Given this equation, Sr(OH)2(s)-Sr2* (aq) + 20H (ag), what is the pH of a 2.5 X 10-4 M Sr(OH)2…

A: Given,  The chemical equation,  Sr(OH)2(s) ------> Sr2+(aq) + 2OH-(aq)  Concentration of Sr(OH)2…

Q: What is the pH of a 0.240 M solution of potassium cyanide? Ka (HCN) = 6.2 × 10-10

A:

Q: What is the pH of a .459 M solution of NaClO. Ka= 2.87x10^-8

A:

Q: The pH of a solution is 3.38. What is the OH concentration in the solution? esc 24 % 4. 6. 7 E R. T…

A: The ph of the solution is 3.38 what is the OH- concentration in the solution

Q: What is the pH of a 0.04 M of the diprotic acid H2CO3 solution? Kal= 4.3 x 10-; Ka2 = 4.8 x 10-11. O…

A:

Q: What is the pH of a 0.04 Mof the diprotic acid H2CO3 solution? Kai= 4.3 x 10-; Ka2 = 4.8 x 1011 %3D…

A:

Q: . Calculate the pH and all the equilibrium concentrations for the complete dissociation of a 5.0M…

A: Arsenic acid is a triprotic acid where H3AsO4 dissociates to H2AsO4- which then further dissociates…

Q: Which kind of intermolecular attractive force is shownin each case here?

A: Part (a): (i) in first case the inter molecular force is Dipole-Dipole force. This is because in HF…

Q: Calculate the pH of a 0.20M c2h5nh2 solution kb=5.6x10^-4

A: Ethylamine(CH2CH2NH2) is a base (because Ethylamine has one lone pair to accept a proton(H+)).…

Q: Calculate the pH of a 0.88M CH3NH2 given Kb= 4.2x10^-4

A:

Q: What is the pH of a solution that has 0.22 M fluoride anion and 0.28 M hydrofluoric acid?  Ka…

A: Given data,Concentration of F-=0.22MConcentration of HF=0.28MKa of HF=5.62×10-4

Q: What is the pH of a 7.1 x 104 M HCIO4 solution? 1 2 3 4 5 C 7 8 +/- х 100

A:

Q: What is the pH of a 0.1 M solution of NaHCO3? For H2CO3 at 25°C, Ka1= 4.5E-7 and Ka2=4.8 E-11. A.…

A:

Q: For the diprotic weak acid H2A, Ka1=2.9×10−6Ka1=2.9×10−6 and Ka2=5.3×10−9Ka2=5.3×10−9. What is the…

A: Ka1 and Ka2 values of a diprotic weak acid are given as 2.9×10-6 and 5.3×10-9 respectively.

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.