Calculate the pH for a 10.0 M solution of NH3 (kp= 1.8x105) NH3 - NH4 + OH a 13.987 O b .013 O c 1.87 O d 12.13

Q: A 0.010 M solution of a weak acid, HA, has a pH of 3.10. What is the K, of the acid? 6.3 x 106 6.3…

A: pH is the negative logarithm of the hydronium ion concentration of a solution. Given:- pH = 3.10…

Q: What is the pH of a solution when 4.9 g of ammonium bromide, NH,Br (M=98) , is used to make 200 mL…

A: Mass of NH4Br = 4.9 g Volume of solution = 200 mL K = 5.6E-10 pH =?

Q: What is the pH of a 0.04 Mof the diprotic acid H2CO3 solution? Kal= 4.3 x 10-/; Ka2 = 4.8 x 10-1.…

A: pH is a measure of acidity and basicity of a solution.

Q: Benzoic acid has a K, of 6.46 (10 5). If I have a 1.668(10) molar solution of benzoic acid, what is…

A:

Q: 10. A 0.045 M solution of hypobromous acid (HBrO) has a pH of 5.02. Calculate the K, for hypobromous…

A: According to the question, the balanced chemical reaction is: HBrO(aq) + H2O(l)   ---->  H3O+(aq)…

Q: What is the [H+] for a 0.010 M HOBr, hypobromous acid, solution?  Ka for HOBr is 2.5 x 10-9. a) 2.5…

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Q: A 0.10 M aqueous solution of the sodium salt of which of the following anions will have the highest…

A: High electronegativity creates a pull for the protons. More electronegative atoms will exert more…

Q: What is the pH of a solution when 4.9 g of ammonium bromide, NH4B (M=98) , is used to make 200 mL of…

A:

Q: The pH of a 0.55 M aqueous solution of hypobromous acid, HBRO, at 25.0 °C is 4.48. What is the value…

A: pH of  HBro = 4.48    -logH+ = pH             H+ =10-pH             H+ = 10-4.48…

Q: A 0.432 M solution of pyridine has a pH of 9.40. What is the K, of pyridine? Oa. 2.7 × 104 Ob. 1.5 x…

A:

Q: 15. Determine the [H3Oʻ] concentration AND the pH of a 5.56 M HCN solution. The Ka for HCN is 5.8 x…

A: The weak acid dissociates into its ions when present in the solution.HCN+H2O↔H3O++CN-Ka=H3O+CN-HCN

Q: 23 What is the pH of a solution composed of 0.20 M NH3 and 0.15 M NH.CI? (Kb NH3 = 1.8 x 10*)" (a)…

A: The pH and pOH of the solutions is the potential of H+ and OH- ions present in the solution. The…

Q: What is the Ka of cyanuric acid if a 0.030 M cyanuric acid aqueous solution has a pH of 4.15? O…

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Q: 12) What is the [H,O'] and pH of a 0.350 M HF solution? The K of HF is 3.5 X 104. HF (aq) + H2O (1)…

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Q: A 0.080 M solution of HX is 4.2% ionized. Calculate K, of this acid. O 3.5 x 104 O 1.4x 10-4 O 3.5x…

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Q: Heroin, a derivative of morphine, is a powerful analgesic and a powerful narcotic agent. Calculate…

A: Heroine is a base.

Q: What is the pH of an aqueous solution that is 0.011 M CH3COOH (Ka = 1.8 x 10-5) and 0.019 M…

A: An aqueous solution containing weak acid (CH3COOH) and it's conjugate base (CH3COONa) results in the…

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

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Q: Calculate the pH of a solution that contains 0.20M of cyanic acid (HCNO) and 0.80 M of sodium…

A: To find pH

Q: What is the pH of a 0.04 Mof the diprotic acid H2CO3 solution? Kal= 4.3 x 10-7; Ka2 = 4.8 x 10-11.…

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Q: The pH of a 0.250 M hypoiodous (HOI) solution is 5.620. What is the value of Ka   a. 5.76 x…

A: Calculate the concentration of hydrogen ions.

Q: What is the pH of a 0.291 M solution of ammonium, a weak acid with a Ką of 5.8 x 10-10? a. 4.89 b.…

A: pH of weak acid is calculated by considering Ka value.

Q: The pH of 0.100 M Jackmanic Acid, HJa, is 2.24. What is the value of Ka for the acid? a. 4.4 x 10-5…

A: Equation representing dissociation of HJa in water: HJa + H2​O → H3​O++ Ja− Dissociation constant,…

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: A solution is made with 3.825 g NH,CI, dissolved in enough water to make 625 mL of solution. If the…

A: First, we calculate the concentration of the solution. After that, we calculate the [OH-] with the…

Q: A solution of CgH5N (pyridine, Kp = 1.7 x 10) has a pH of 9.40. What is the [C;H5N]? O 0.37 9.3 x 10…

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Q: Calculate the pOH of a 0.20 M solution of pyridine, C5H5N. The Kb value for C5H5N is 1.7 x 10-⁹. O…

A: we have to calculate the pOH of 0.20 M pyridine

Q: Calculate the pH in an aqueous solution which is 0.125 M NH3 and 0.300 M NH4CI. The value of K is…

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Q: 4. Solution of 0.1 M NaHSO4 a. Equilibrium reaction b. Equilibrium constant expression: Ka = 1.2 x…

A: using the ionic equilibrium, kb=kwkakw=1.0×10-14ka=1.2×10-2   Kb=0.833×10-12 using this find the…

Q: Consider an initial 0.040M hypobromous acid (HOB) solution at certain temperature. HOBr H*(0) +…

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Q: What is the pH of a 4.8 M pyridine solution that has Kp = 1.9 x 109? The equation for the…

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Q: I C E Determine the pH of a 0.095 mol/L HIO4 solution if the K₁₂ = 1.29 x 10-² + H₂O (l) HIO4 (aq)…

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Q: A 0.030 M aqueous solution of a sodium salt (NaA) has a pH of 8.23. What is the value of K, for the…

A: The correct answer is given below

Q: What is the pH of a o.725 M carbonic acid (H,CO,) solution given Kal = 4.4 × 10-7 and Ka2 = 4.7 ×…

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Q: Calculate the pH of the solution. Assume 1.0 L of solution. You must identify the type of solution…

A: There are two types of bases/acids. One is strong base/acid which is completely dissociable in into…

Q: (Q13) The poison strychnine is a weak base with Kp = 1.8 x 106. What will be the equilibrium pH of a…

A: Given-> Kb = 1.8 × 10-6 Molarity = 0.710 M

Q: The Ką of hypochlorous acid (HCIO) is 3 x 108. What is the pH at 25.0 °C of an aqueous solution that…

A:

Q: 8. What is the pH of a 0.20 M solution of sodium acetate? The K, for acetic acid is 1.8 x 10-5 ?

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Q: Formic acid is in the venom of some ant species. What is the pH of a 0.35 M solution of formic acid…

A: Given: Concentration of formic acid HA = 0.35 M And Ka of HA = 1.78 × 10-4  The dissociation…

Q: Calculate the pH of a 0.383 M NH, solution. NH, has a Kp 1.8 x 10-5. pH

A: NH3 is a weak base and since Kb value is very less so it is assumed that reaction proceeds very less…

Q: A 0.75 M solution of a certain weak base has a pH of 11.60. What is the K, for this weak base? O 3.6…

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Q: Suppose sodium hydroxide is added to a 0.Q120 M solution of zinc nitrate such that the pH of the…

A: The given data contains, Concentration = 0.0120 M. pH = 13.1

Q: A flask of 0.70 M HBrO2(aq) has what pH? (Ka = 1.2 x 10-5) A 2.18 B 2.16 C 3.20 D 2.66 E 1.90

A: Given data contains, Molarity of HbrO2 is 0.70 M. Ka is 1.2 x 10-5.

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 solution that is 0.053 Min HA and also 0.063 Min NaA? (Ka = 4.1 × 10-6) 5.46 O…

A: Henderson Hasselbalch equation, pH = pKa + log [salt]/[acid]

Q: 5. Determine the pH of the solution which has 10% of NaOH in deionized water by mass. The NaOH which…

A: Given that -  Mass percentage of sodium hydroxide, NaOH = 10%.  Density of this Solution = 1.131…

Q: What is the pH of a 0.31 M solution of NH4CIO4? Kp of NH3 is 1.8 x 105. Round tenth (X.X).

A: given data from question- conc. = 0.31 M Kb = 1.8×10−5 pH = ?

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: The pH of a solution containing 0,1 M of a weak acid HA is 6. Calculate Ka for this acid. O 1.0 x…

A: Let HA is a weak acid whose concentration is 0.1 M and pH is 6 and the dissociation constant is Ka.…

Q: /hat is the largest difference between the Arrhenius and Bronted Lowry acid/bas efinitions? 0.05 M…

A: Since you have posted multiple questions so as per guidelines we can answer one per session . If you…

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.