What is the pH of 3.7 x 103 M NH¼Br(aq)? Ο 10.4 O 2.4 Ο 11.7 O 5.8 O 4.6

Q: What is the pH and pOH of a 28% KH2PO4?

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Q: What is the pH of a 0.45 mol/L solution of hydrobromic acid? The answer should be to the proper…

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Q: What is the pH of .08 M H2SO3 (aq)? O 12.51 Ο 1.10 0 .94 O 1.89 Ο 1.49

A: Concentration of H2SO3 = 0.08 M  pH of the H2SO3 = ?

Q: When fermentable carbohydrates are left in the mouth, bacteria in the mouth produce an acid with a…

A: The formula of hydronium ion is H3O+. pH is the negative log of hydronium ion concentration. The…

Q: Calculate the equilibrium concentrations of all chemical species present in a 0.10 M H2CO3(aq)…

A: Dissociation of H2CO3 takes place as follows: Since H2CO3 is a weak acid, thus x can be neglected…

Q: What is the pH of a 0.0470 M solution of methylamine (CH&NH2, Kb = 4.4 x 10 4)?

A: Calculate the hydroxide ion concentration released by methylamine. OH- = KbCOH- = 4.4 × 10-4 ×0.047…

Q: The pH of a solution containing a [H3O+] = 3.40 x 10 negative 5 M, is:

A: pH is a scale to measure the concentration of hydrogen ions. The negative logarithm of hydrogen ion…

Q: In what terms can you express the alkaline strength of pearl ash?

A: Pearl ash is also known as potash, chemically it is potassium carbonate.

Q: What is the pH of a 0.012 M Ca(OH)2 solution? O 12.38 O 1.62 O 1.92 12.08

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Q: What is the pH of a 0.100 M solution of LiBrO(aq) at 25'C? Assume that LiBrO is a strong…

A: Since you have posted multiple questions, we are entitled to answer the first only. Given:…

Q: 2. Describe the variation of the acid strength for the hydrogen halide series and explain which one…

A: Arrange the acids in increasing order of acidic strength--

Q: 7. What is the pH of a 0.025 mol/L solution of methanoic acid? K₁ = 1.8 x 104

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Q: What is the pH of a 0.21 M solution of methylamine (CH3NH2, Kb = 4.4 x 10–4) at 25 degrees C?

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Q: 12. What is the pH of a 1.00 molar solution of NaNO2(aq)? The K, for nitrous acid is 7.0 x 104. a.…

A: NaNO2 is a strong electrolyte that dissociates completely in water. Its ionic component NO2- gets…

Q: Calculate the pH and pOH of: 0.3M sulfuric acid (H2SO4) solution

A: Given:  Molarity of H2SO4=0.3M

Q: What is the pH of a 0.35 M solution of trimethylamine, (CH3),N (Kb = 7.4 x 10 5)?

A: Given : concentration of (CH3)3N solution = 0.35 M  Kb for (CH3)3N = 7.4 × 10-5  To calculate :-  pH…

Q: What is the pH of .03 M NH4Br (aq)? O 3.13 O 9.25 O 10.87 O 1.52 O 5.38

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Q: The pH of an aqueous solution of 0.061 M ascorbic acid, H2C,H606 (aq), is

A: Please find your solution below : pH is the measure of extent of H+ concentration and the extent of…

Q: culate the pH of an 3.09 x 103 mol/L solution of hydrochloric acid to two wer:

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Q: The pH of a lime is 1.90. What is the [H3O*]?

A: Power of hydrogenpH value indicates the acidic and basic nature of a solution. pH ranges between 0…

Q: .Write a balanced equation for the dissociation of each of the following Bronsted- Lowry acids in…

A: Bronsted-Lowry acid-base theory: The Bronsted-Lowry acid-base theory states that the acid is a…

Q: What is the pH of .15 M KBRO(aq)? O 3.07 O 4.75 O 13.18 O 9.25 O 10.93

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Q: what is the pH of a 0.15 mol/L solution of hypochlorous acid? the answer should be written to two…

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Q: The pH of an aqueous solution of 9.43x102 M tellurous acid, H,TeO3 (aq), is For H,TeO3 K =5.40*10…

A: Dissociation of tellurous acid is, Ka1 and Ka2 values of a tellurous acid are given as 5.40×10-7…

Q: What is the pH of 5.35 x 103 M H2CO3 (aq)? O 4.3 O 8.6 O 2.3 O 4.9 O 9.1

A: Concentration of H2CO3 = 5.35 × 10-3 M  pH of the H2CO3 = ?

Q: What is the pH of 7.8 x 105 M HNO3 (aq)? O 18.1 O 9.9 O 9.5 O 3.7 O 4.1

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Q: 5. A solution is initially 0.050 M in ammonia, NH3 (Kp = 1.8 x 10°). (a) Write the equilibrium…

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Q: What is the pH of .76 M CN (aq)? O 13.9 O 4.7 O 9.3 O 2.4

A: Interpretation : We have to calculate the pH of CN- .

Q: Calculate the pH of 0.10 M (COOH)½ (aq), oxalic acid. Ka1 = 5.9 x 10-² ; Ka2 = 6.4 x 10-5.

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Q: What is the pH of 6.3 x 10-4 M Ba(OH)2 (aq)? Ο 11.1 O 10.8 O 3.2 O 2.9 O 7.6

A: We have to calculate the pH of 0.00063M Ba(OH)2 solution.

Q: Place the following acids in order of increasing strength: -H​3P​O​4,​ H3P​O​2​ and H3P​O​3.​…

A: We have to explain the acidity order: -H​3P​O​4,​ H3P​O​2​ and H3PO3.

Q: What is the pH of .03 M HC2H3O2 (aq)? O 10.07 O 1.52 O 4.74 O 3.13 O 6.27

A: Ka is acid dissociation constant which determines strength of acid. Stronger acid dissociates more…

Q: The pH of an aqueous solution of 0.0327 M ascorbic acid, H,C,H,O6 (aq), is

A: The solution is as follows:

Q: What is the pH of a 2.85 M , solution of HNO3 (aq)?

A: pH is defined as the negative logarithm to the base 10 of H+ ion concentration expressed in mol/L pH…

Q: Why is rainwater naturally acidic, even in the absence ofpolluting gases such as SO2?

A: Acidic substances are those substances that have a pH value is in the range of 0 to 7. When the…

Q: What is the pH of .242 M H2CO3 (aq)? O 6.38 О 3.50 O 10.50 O 4.12 O 5.47

A: pH is defined as negative log of concentration of H+ ions in the solution.

Q: 7. What is the pH of [H30+]= 2.4 * 103 M? O 2.6 O 2.4 O -3 O 5.4

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Q: Calculate the pH and percent ionization of a 2.5 x 102 45 x 10:4)

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Q: Determine the pH of a 0.450M solution of aniline hydrochloride. C6H;NH, (ag) + H,O(1) = H;O* (ag) +…

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Q: How many times more acidic is battery acid with a Ph of 0 than tomatoes with a Ph of 4?

A: Given: pH of battery acid = 0  And pH of tomatoes = 4

Q: Given that methylamine, CH3NH2, has a Kb of 4.4 x 10-4, what is the pH of a 0.20 M aqueous solution…

A: For weak base CH3NH2 : [OH-] = Kb×C          = 4.4×10-4×0.20           = 9.38 x 10-3 M pOH = - log…

Q: What is the pH of a 1.63 M solution of XOH, a weak monobasic compound (Kb = 1.7 x 10^-9)?

A: Given data in above Concentration of XOH = 1.63 M  Kb = 1.7 ×10-9

Q: What is the conjugate acid for H_2SO_3(aq)?

A: The pair of acid and base differing from each other by just one proton is called conjugate acid-base…

Q: Calculate the pH of 1.00M acetic acid, HC2H3O2(aq). (Ka = 1.8 x 10-5)

A: Dissociation constant, Ka = 1.8 x 10-5 Concentration of acid = 1 M

Q: Calculate the pH of 0.400 M solution of ascorbic acid, HC6H;O6. (Ka of ascorbic acid = 6.80 x 105)

A: In this question, we want to determine the pH of this solution. How we can determine, you can see…

Q: The K, for hypoiodite anion (IO) is 4.35x10-4. What is the pH of a 0.226 mol L solution of lithium…

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Q: The pH of 0.01 m Potassium hydrogen phthalate is... O 2.05 O 3.55 O 4.00 O 5.00 O 6.00

A: Here we are required to find the pH of the solution of 0.01M of KHP.

Q: How many moles of hydroxide ions can be released into solution from 1.00 mg of Mg(OH)2 that is used…

A: Molar mass of Mg(OH)2 = 58.32 g/mol Given mass = 1 mg = 0.001g Moles = 0.001/58.32 = 1.71*10-5

Q: The pOH for O.2 M sulfuric -2 acid solution is

A: We have 0.2 M sulfuric acid H2SO4 solution.we need to calculate the pOH of this solution.

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.