What is the pH of a 0.02M ammonia solution if its Kb va www H.O + NH, 0H + NH,. O 3.2 O 12.3 O 10.8 76

Q: The ionization constant for ammonia is 1.8 x 10-5. What is the pH of an aqueous solution labeled…

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Q: What is the pH of 6.0 x 104 M HF? The K, for hydrofluoric acid is 7.2 x 104. O a. 2.95 b. 3.22 C.…

A: Answer:- This question is answered by using the simple concept of ionisation of weak acid and then…

Q: 19) Calculate the pH of a solution (aq., 25 °C) prepared by dissolving 48.026 g of ammonium nitrate…

A: Given:   Mass of NH4NO3=48.026g   Molar mass of NH4NO3=80.043 g/mol   Volume =2.00L…

Q: The pKa for HCN(aq) is 9.21. What is the pH of a 1.245 M solution of NaCN? O a. 11.25 O b. 1.24 O c.…

A: this is the salt of weak acid and strong base. so ,we will use hydrolysis equation of weak acid and…

Q: Calculate the pH of a solution when 21.0 mL of 0.050 M hydrazine (N2H2, Kb=8.9E-7) is titrated with…

A: pH of a weak base titration with strong acid can be determine using Henderson hasselbalch equation.

Q: What's the pH of the solution? See attached image. Please show steps.

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Q: 10) What is the pH of a 0.100 M NH3 solution that has Kb = 1.8 × 10-5? The equation for the…

A: For the reaction

Q: Determine the |H*|,|OH¯|, and pH of a solution with a pOH of 3.82 at 25 °C. [H*] = %3D M [OH] = M pH…

A: Here , we use the equilibrium formula , that is [H+]=[OH-]= 10^-7, and pH+pOH = 14 at 25 degree…

Q: Formic acid (HCHO,) has a K, 1.8 x 10. What is fractional composition (a) of formic acid in solution…

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Q: What is the pH of a 0.060 M Ba(OH)2 solution at 25 °C? D 8.08 D 1.92 D 12.78 13.08 1.22

A: pH :-        It is a scale to measure the acidic or basic nature of any substance.    Given data in…

Q: Calculate the pH of solution made by combining 100 ml of 0.28 M HC,H;O2 and 50 ml of 0.36 M NaOH, Ka…

A: Since there is mixing of weak acid and strong base so it is a case of acidic buffer. The pH can be…

Q: 4. Calculate the pH and pOH of each of the following solutions. a. [H*] = 1.0x10-M ph= 4,poh=10 =14…

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Q: 28. What is the pH of a 0.62 M NH,NO, solution at 25°C? [Kb for NH; is 1.76 × 10°] А. 2.48 В. 4.73…

A: Welcome to bartleby !  We have to calculate pH

Q: The pH of a 0.50 M solution of the weak acid HA is 4.76. The value of Ka is O a. 6.0 x 10-10 O…

A: Given data :- Concentration of weak acid = 0.50 M pH of weak acid (HA) = 4.76

Q: The pH of a 0.063-M solution of hypobromous acid (HOBr but usually written HBrO) is 4.95. calculate…

A: Given: pH of hypobromous acid, HOBr = 4.95 Concentration of HOBr acid = 0.063 M Ka = ?

Q: Calculate the concentration of all the species present, the pH and the percent dissociation of…

A: We have 0.15 M NH3 and 0.45 M ammonium ion concentration , we have to predict concentration of all…

Q: 28. What is the pH of a 0.62 M NH;NO3 solution at 25 °C? * [Kb for NH, is 1.76 × 10*] A. 2.48 В.…

A: Ammonium nitrate is a slat of weak base, ammonium hydroxide and strong acid, nitric acid.…

Q: Calculate the pH of an aqueous solution of 0.70 M H3BO3 and 0.40 M H;BO3 Acid Formula Ka pKa HCOOH…

A: Henderson - Hasselbalch equation:

Q: Calculate the pH of 0.030 M Ba(OH), solution. 12.78 O 1230 O 122 O 12.48 12.16

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Q: Calculate the pH of HOCI solution that is 2xE-6 M, Ka =2.8xE-8 а. 2.8 O b. 2.4 O c. 1.3 O d. 6.6

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Q: What is the pH of a 0.481 M solution of NH4Br? For NH3, Kb = 1.8 × 10–5

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Q: If the kb NH3 = 1.8x10^-5, calculate the mass of NH3 in a 1.0 L ammonia solution whose pH is 11.10

A: Ammonia is weak base hence it dissociated less in aqueous solutions

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 IxE-9 M HCI solution? O a. 6.99 O b. 9.00 Oc. 9.1 O d. 7.5

A: Answer: option b. 9.00 is the pH of the HCl solution.

Q: What is the pH of a 0.100M NH3 solution? Kb for NH3 is 1.8 x 10-5? NH3(aq) + H2O() = NH4+(aq) +…

A: NH3 is a base and NH4+ is its conjugated acid. pKb of ammonia is 1.8×10-5. The dissociation of NH2OH…

Q: The poison strychnine is a weakly basic compound with Kb = 1.8 x 10 What is the pH of a 0.058 M…

A: Given that, 0.058 M solution of a weak base, i.e. C = 0.058 M. The Kb is 1.8×10-6. We have to…

Q: what is the ph of a solution with (H3O+) = 2.8 *10^-9 M? a. -8.6 b. -5.4 c. 3.6 *10 ^-6 d. 5.4…

A: pH = -log(H3O+)

Q: What is the PH of a 0.500 M NACIO solution? K, of HCIO is 2.9x10-8 O a. 9.48 b. 4.52 O c. 10.62 O d.…

A: NaClO → Na+ + ClO- ClO- →HClO + OH- Now , let [HClO] =[OH-] = X  So , Kb = [HClO]×[OH-]/[ClO-] =>…

Q: 13. What is the pH of a 0.0 1 5M Ca(OH)2 solution? a. 1.52 b. 12.18 c. 12.48 d. 1.82

A: The required equation is given below.

Q: What is the pH of a 0.65 M solution of pyridine, C5H5N? (a) 4.48 (b) 8.96 (c) 9.52 (d) 9.62 (e) 9.71

A: Given,  The concentration of C5H5N is 0.65M The kb value of C5H5N is 1.7×10-9   To solve: pH of…

Q: What is the concentration (in M) of hydroxide ions in a solution at 25.0 °C with pH = 4.186? O 1.53…

A: Given: pH=4.186 [H+]=6.52×10-5 Formula used: pH=-logH+H+OH-=10-14

Q: A solution with an OH| concentration of 1.20×10-7M has a pH of O 7.06 O 7.07 O 7.08 7.09

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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 a 0.31 M sodium formate solution (HCOONa).   Kb for HCOO− = 5.9 × 10−11

A: Given :-  [HCOONa] = 0.31 M  Kb for HCOO- = 5.9 × 10−11  To calculate :-  pH of solution

Q: The Ka for formic acid (HCO2H) is 1.8 · 10 What is the pH of a 0.45 M aqueous solution of sodium…

A: pH is a measure of acidity and basicity. The range is 0 to14. When pH is 7, solution is neutral. pH…

Q: Calculate the pH of a 0.645 M NH3 solution.NH3 has a ?b=1.8×10−5

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Q: What is the pH of 500.0 mL of a 0.1 M NaOH solution? O A. 13 О В. 1 ОС. 1.3 O D. 12.7 47L Ansuers to…

A: Given :  Concentration of NaOH solution  = 0.1 M

Q: Which one has the highest pH? pks values CSHSN 8.77 CH:NH2 3.36 NH:OH 7.96 CeHsNH2 9.41 N2H4 5,89

A: Acid is a substance which donates H+ ion when dissolved in water.  Base is a substance which accepts…

Q: What is the pH of a 0.02M ammonia solution if its Kb value is 1.8*10^.5? H.O + NH, 2 OH + NH,. 3.2 O…

A: The value of Kb for the given weak base is = 1.8×10-5 The concentration of the base solution is =…

Q: Find the pH of 0.175 M NaCN solution. For HCN,Ka = 4.9 * 10-10.a) 5.03 b) 11.28 c) 2.31 d) 8.97

A: pH is the negative logarithm of concentration of hydronium ion (H3O+).…

Q: What is the pH of a 0.02M ammonia solution if its Kb value is 1.8*10^-5? H,O + NH, 2 OH- + NH,. 3.2…

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Q: The [H3O+] in a 0.005 M solution of Mg(OH)2 is: * O (a) 1.0 x 10-12 M O (b) 2.0 x 10-12 M O (c) 1.0…

A: MgOH2  → Mg2+ + 2 OH-OH- = 2 × 0.005M = 0.01 MWe know thatKw = H3O+OH-    ....(ionic product of…

Q: please highlight the correct answer

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Q: B. What is the pH of 0.75 M HC:H3O2 solution? K.= 1.8 x 105 and Kw=1.00 x 10-14 HC:H3O2 + H2O H30 +…

A: Calcuation as shown below

Q: What is the pH of a 3.1 x 10-3 M LiOH solution? a. 11.5  b. 2.51 c. 11.2 d. 2.64

A: To calculate the pH of an aqueous solution you need to know the concentration of the hydronium ion…

Q: 7. A solution with pH of 9.50 has a pOH of А. 9.50 О В. О.50 Ос. 4.50 D 11 3

A: pH  is a scale used to specify the acidity or basicity of an aqueous solution. Acidic solutions  are…

Q: What is the pH of a solution of 0.010 M CH3NH3ClO3?    A. 8.54  B. 6.32 C.4.74 D.10.12

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Q: 7. Aniline (C6H5NH2) has a Kb of 3.8 x 10-10. What is the pH of a 0.150 M aniline solution? (a) 5.12…

A: Given,Concentration od aniiline  = 0.150M.Kb of aniline = 3.8*10-10.

Q: Calculate the pH of a 0.048 M solution of the following compounds. NH3. Kp(NH3) = 1.8E-5. eTextbook…

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Q: * At a temperature where the ionization constant is 1x10 ^-8 What is the PH value of a 1000 µL…

A: A weak monoprotic acid will ionize as follows in its aqueous solution HA⇔H+(aq)+A-(aq)C--C-CαCαCα…

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.