Calculate the pH and [S2-] in a 0.10-M H2S solution. Assume Ka1 =1.0×10-7; Ka2 = 1.0×10-19.

Q: Determine the Kb of a weak base if a 0.31 M solution of the base has a pH of 11.79 at 25°C.

A: The pOH is calculated from pH as shown below.

Q: Calculate the pH and pOH of a solution at 25°C, if [OH-] = 5.3 x 10-7 M. Answer to the hundredths…

A: pH and pOH can be calculated as follows

Q: Consider H3A a triprotic acid with Ka1 = 3.0 x 10-3, Ka2 = 5.6 x 108 and Ka3 = 8.1 x 10-13, %3D %3D…

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Q: Calculate the pH of a 0.10 M HCOOH solution. Ka of HCOOH is 1.8 X 10-4.

A: pH is defined as the negative logarithm of hydrogen ion concentration present in the solution.…

Q: Calculate [H+] and pH in a solution in which [HNO2] is 0.10 M and [NO2:] is0.20 M. Given Ka = 4.5x…

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Q: Match the 0.10 M aqueous solution to the approximate pH range. HNO3 1. pH under 2 CH3NH3B

A: Acids are substances that donate protons in aqueous solutions whereas bases are substances that…

Q: Calculate the ph of the [OH-] = 2x10^-3 M.

A: We have to calculate the pH of given solution.

Q: Calculate the pH of a solution with a [H 30*]=5.6x10 -9 M.

A: Formula to calculate pH :- pH = -log[H3O+]

Q: What is the pH of a 0.087 M solution of H2SO4? Round to two decimal places.

A: Given, Concentration of Sulfuric acid = 0.087M

Q: what is the pH when the H3O concentration is 0.0003M?

A: The pH of a solution can be calculated as given below.

Q: Consider a solution that contains both NH3 and NH4NO3. If a solution has a pH of 7.70, calculate the…

A: When a solution contains weak base and its salt with strong acid, a buffer is formed. Such a…

Q: Determine the [H*],[OH-], and pOH of a solution with a pH of 13.34 at 25 °C. H*] 4.571 x10-14 OH] =…

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Q: em101 The pH of a 0.0049 M solution of Ca(OH), is

A: Given that: molarity of Ca(OH)2 = 0.0049 M To find: pH of 0.0049 M Ca(OH)2 solution?

Q: What is the pH of a solution with [H3O+]=1x10-9M?

A:

Q: Determine the pH of a 0.65 M solution of HCO₂K. The value of Ka for HCOOH is 1.8 × 10⁻⁴.

A: HCOOK is a salt of a weak acid (HCOOH) and a strong base (KOH). The salt is present as HCOO- and K+…

Q: What is the pH of a solution that has [OH-] = 5.0 x 10-7 M?

A:

Q: What is the pH of a solution at 25 C if the [OH-] = 5.0 x 10-3 M?

A: pH measures the acidity of a solution. If pH is greater than 7 then solution is basic. If pH is less…

Q: Calculate the OH- concentration for a solution with a pH of 3.66

A: Since pH = 14 + log[OH- ]  where [OH- ] = concentration of OH-  ion

Q: Determine the [H+][H+] , [OH−][OH−] , and pOH of a solution with a pH of 13.4113.41 at 25 °C.

A: Answer: [H+] = 3.89 × 10-14 M , [OH-] = 2.57 × 10-1 M and pOH = 0.59

Q: Determine the OH, pH, and pOH of a solution with a [H*| of 8.7 x 10-8 M at 25 °C. |OH] = %3D pH =…

A: The following formulas will be used here, pH= -log[H+] pH + pOH = 14 [H+][OH-]=10-14   Given, [H+] =…

Q: Determine the [H*], [OH-], and pOH of a solution with a pH of 13.23 at 25 °C. [H*] =

A:

Q: Find the pH of a 0.200 M NH4Cl solution given that the Kb of NH3 = 1.8x10-5 at 25 °C.

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Q: Determine the H*|, pH, and pOH of a solution with an OH-] of 4.2 x 10-12 M at 25 °C. [H*] = M %3D pH…

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Q: the [OH^-] was measured to be 5.60 x 10^-10 M then what is the pH

A:

Q: Q49 (Ex. 13.6) In chemistry, the pH value . measure.. acidity. The pH value is defined by pH where…

A: pH :-  It is defined as the negative logarithm to the base 10 of hydrogen ion (H+ ion )…

Q: Calculate the pH of a 0.36M methylamine (weak base) (CH3NH2) solution, if Kb = 4.4x10-4

A: In aqueous solution, methylamine undergoes the acid base reaction: CH3NH2 aq + H2Ol  → CH3 NH3+ +…

Q: CALCULATE THE [H30+] CONCENTRATION OF A SOLUTION WITH A PH OF 5.5

A: Given pH = 5.5

Q: 2. Given the following values for the apparent pH, find (H*) in the following solutions: (a) pH = 0…

A: The pH of any solution shows that the solution is acidic or basic.  For multipart questions, we are…

Q: Hydrazine, N2H4, has Kb = 1.3E-6. Calculate the pH of a 0.644 M solution of N2H4.

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Q: Calculate the pH and pOH of a solution at 25°C, if [OH-] = 1.3 x 10-⁹ M. Answer to the hundredths…

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Q: Choose the CORRECT statement(s) regarding 0.0010M NH: solution. [Kb NH3= 1.8 x 10-] * The…

A:

Q: What is the pH of a solution that has [OH–] of 5.15×10-3 M ?

A: Given, Concentration of hydroxide ion = 5.15×10-3 M

Q: Calculate [H30*] of a solution with a pH of 5.5

A: Given information: pH of solution = 5.5

Q: If the pH of a solution is 6.8, calculate [H*]. O 2511.886431510 O 0.000398107 O 0.000000158 O…

A: Relation between pH and H+  pH = -log[H+]  We want to determine [H+] concentration  -pH = log[H+]…

Q: Calculate [H3O+] in a solution that has [OH-] =6.7 X 10-2 M at 25C. Is the solution neutral, acidic,…

A: For aqueous solution, the product of the concentration of hydronium and hydroxide ions is given by:…

Q: find [OH-] and [H3O+] if the pH= 2.75

A:

Q: Which would have a more basic pH, a solution whose hydrogen ion concentration is 1.0 x 10^-12 M or a…

A: We know that pH is the negative logarithm of the concentration of Hydrogen ion.  pH = - log [H+] And…

Q: What is the pH of a solution containing 0.453 mol L-1 HF and 0.267 mol L-1 F- ? Round your answer to…

A: Given,  [HF] = 0.453 M  [F-] = 0.267 M  What is the pH of the solution = ?

Q: Hydrazine, N2H4 has Kb= 1.3E-6. Calculate the pH of 0.486M solution of N2H4.

A: Hydrazine is a weak base.We have to calculate pH given hydrazine solution. Recall the following…

Q: if the H3O+ ion concentration in an aqueous solution at 25 °c measured 4.61 * 10^-8 M, what is the…

A: Given : [H+] = 4.61 * 10^-8 M

Q: For questions 7-9 state which species (chemical) is the acid, which is the base, and which are the…

A: Bronsted Lowry acid-base theory. Acid is the chemical species that donates protons in the solution…

Q: Find the pH of a 0.247 M NH4Cl solution given that the Kb of NH3 = 1.8x10-5 at 25 °C. 11.32 2.68…

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Q: [H+] = .0001 [H+] = 0.0030 [ОН-]— 8.6 е -8 РОН %3D 4.9 pH = 7.3 II At 37 degrees C, which of these…

A: We have to predict the solution that is nearly neutral.

Q: 1. The formula for the conjugate acid of C20, is 2- 2. The formula for the conjugate acid of HPO, is

A:

Q: Determine [OH-] and pH of a solution that is 0.140 M in F- .

A: Given, concentration of solution with F- is 0.140M.The reaction of fluoride ion with water can be…

Q: Calculate the pH of a solution if [H*] is measured to be 5.76 x10-9 M. Is this solution acidic or…

A: Given: Concentration of [H+] ion = 5.76×10-9 M

Q: Calculate the pH of the following aqueous solution:           0.62 M H2S (pKa1 = 7.00; pKa2 =…

A: H2Saq⥪H+aq+HS-aq                                       pKai=7.00                PKa1=-log Ka1…

Q: Determine the pH of the following solutions at 25°C. (a) [H,0']-7.36 x 10 10M pH M 10 *72א - [ 9,0]o…

A: The pH of the solution is calculated using the following formula: pH=-logH3O+ ......(1)

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.