You have to calculate the pH of 0.020 M NH3 (Kb = 1.75 x 10-5). a- Write the four equations to solve this problem. b- Simplify the algebra by making two reasonable assumptions and calculate the pH. c- Verify if both assumptions are accepted when the error introduced by each assumption is less than 5%.

Q: Calculate the pH and concentrations of CH, NH, and CH, NH; in a 0.0443 M methylamine (CH, NH,)…

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Q: What is the pH of a 0.16 M NH3 solution? Kb = 1.8 x 10-5 (at %3D the current temperature) IMPORTANT:…

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

A: In this question, we want to determine the pH of a solution.  You can see details Solution below…

Q: Calculate the pH of the methylammonium chloride salt (CH3 NH3+ Cl-) 0.3 M. Write the hydrolysis…

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Q: A solution is prepared at 25 °C that is initially 0.11 M in dimethylamine ((CH,) NH), a weak base…

A: [(CH3)2NH] = 0.11 M [(CH3)2NH2Cl] = 0.44 M Kb = 5.4 × 10-4

Q: -4 A solution is prepared at 25 °C that is initially 0.30 M in methylamine (CH, NH,), a weak base…

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Q: A solution is prepared at 25 °C that is initially 0.45 M in chlorous acid (HCI0,), a weak acid with…

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

Q: Can you please further explain to me what I have to do to find the theoretical pH? I’ve prepared a…

A: Given question to calculate the pH of acetic acid solution.

Q: A solution is prepared at 25 °C that is initially 0.13M in methylamine (CH3NH₂), a weak base with…

A: pH for buffer Solution can be calculated using Henderson Hasselbalch equation as follows:

Q: 5,A weak acid, HA, with a molarity = 0.180 M was found to have a pH = 4.54.  Calculate the…

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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: A solution is prepared at 25 "C that is initially 0.89M in trimethylamine ((CH), N) a weak acid with…

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Q: A solution is prepared at 25 °C that is initially 0.48 M in trimethylamine ((CH;),N), a weak base…

A: Given : Concentration of weak base (CH3)3N = 0.48 M Concentration of conjugate acid salt of base i.e…

Q: You are studying a clear solution and you added the pH indicator methyl violet. The colour range of…

A: The color of a solution of pH 0.2 is needed to be determined on the addition of an acid-base…

Q: A solution is prepared at 25 °C that is initially 0.27 M in chlorous acid (HCIO2), a weak acid with…

A: Given  [HClO2] = 0.27 M [KClO2] = 0.19 M Ka of the weak acid, HClO2 = 1.1x10-2

Q: What is the pH of a solution that is 0.20 M potassium cyanate, KCNO and 0.16 cyanic acid HCNO? The…

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Q: 3a.) The Ka of acetic acid is 1.8 x 105. Calculate the pH of the following solutions: a. A solution…

A: The solution mentioned here is a buffer as it is comprised of a weak acid and its salt. As per the…

Q: A solution is prepared at 25oC that is initially 0.42 M in a “X” base, a weak base with Kb =…

A: Since the solution is having base X with concentration 0.42 M and its conjugate acid salt with…

Q: Phosphoric acid, H, PO,(aq), is a triprotic acid, meaning that one molecule of the acid has three…

A: A triprotic acid is an acid that has three dissociable protons. When such an acid undergoes stepwise…

Q: A solution (total volume = 1L) of 0.4 M NH3 contains 12.78 g of NHẠCI (MW = 53.491 g/mol). Kb = 1.8…

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Q: . If BaCl2 completely dissolves in water, what is the ionic strength of a 0.0300 F solution of…

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Q: A solution is prepared at 25 °C that is initially 0.16M in ammonia (NH,), a weak base with K, =1.8 ×…

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Q: In the laboratory, a general chemistry student measured the pH of a 0.559 M aqueous solution of…

A: We have to calculate the value of Ka for formic acid

Q: A solution is prepared at 25 °C that is initially 0.41 M in chloroacetic acid (HCH2CICO2), a weak…

A: Step 1: Step 2: Step 3: Step 4:

Q: 2. Determine the pH if I add 0.5 moles of NHẠC1 (s) to a 5 L solution of water. (Note: the Ka of…

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Q: Can you please fill out the ice table and find the Ka

A: ICE tableKa          Explanation:Step 1: ICE tableICEHC3H5O2 (aq)H2O (l)⇌H3O+ (aq)C3H5O2-…

Q: of A chemist titrates 160.0 mL of a 0.6207M nitrous acid (HNO,) solution with 0.2996M KOH solution…

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Q: A solution is prepared at 25 °C that is initially 0.17M in ammonia (NH3), a weak base with K = 1.8 ×…

A: Solution that  contains weak base (ammonia) and corresponding salt (ammonium chloride) of strong…

Q: A solution is prepared at 25 °C that is initially 0.31M in propanoic acid (HC,H,CO,), a weak acid…

A: Given, Concentration of propanoic acid (HC2H5CO2) = [HC2H5CO2] = 0.31 M Concentration of potassium…

Q: The acid dissociation constant K, of carbonic acid (H,CO,) is 4.5 x 10 '. a Calculate the pH of a…

A: Given Ka for H2CO3 = 4.5 × 10-7  initial Concentration = 0.41 M

Q: Calculate the pH of a 6.00×10-1 M aqueous solution of hydroxylamine hydrochloride (HONH3Cl). (For…

A: The question is based on the concept of salt hydrolysis. we have to calculate pH of given…

Q: The pH of a 0.200 M solution of the weak base pyridine, C5H5N, is 8.59. Draw up a reaction table for…

A: The ionisation reaction of weak base C5H5N can be written as  => C5H5N (aq) + H2O (l) ------>…

Q: What is the pH of a 5.50x10-2 mol L-' ammonia solution? Express your answer numerically to two…

A: Weak base degree of dissociation (α)  can be calculated by the given below formula α  = KbCwhere…

Q: A solution is prepared at 25 °C that is initially 0.37 M in nitrous acid (HNO,), a weak acid with K,…

A: Since the pH of monoprotic acid buffer is given by Henderson-Hasselbalch equation as  where pKa =…

Q: A solution is prepared at 25c that is initially 0.16M in trimethylamine ,( (CH^3)3N) a weak base…

A: Molarity of CH33N = 0.16 M Molarity of CH33NH+ = 0.17 MKb = 7.4×10-4

Q: 0.21 M CH3NH3I (Kp (CH3NH2) = 4.4 × 10-4)

A: Given data: Dissociation constant of base (Kb) = 4.4 x 10-4  Concentration of CH3NH3I = 0.21 M…

Q: Calculate the pH of 0.30 M methylamine, CH3NH2, which has a Kb of 4.4 x 10-4.

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Q: A solution is prepared at 25 °C that is initially 0.38M in methylamine (CH3NH₂), a weak base with K₁…

A: Given,Molarity of methyl amine ( CH3NH2 ) = 0.38 MMolarity of methyl ammonium bromide ( CH3NH3Br ) =…

Q: A solution is prepared at 25 °C that is initially 0.44 M in methylamine (CH, NH,), a weak base with…

A: Methylamine is weak base and Methyl ammonium bromide is its salt.so the solution is buffer solution.…

Q: A 0.763 M solution of a weak acid (HA) is made.  The solution has a pH of 5.32. Calculate the Ka of…

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Q: After dissolving HCI in water, the final concentration of H3O* is 3.87x10-1. What is the pH of this…

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Q: A chemist titrates 180.0 mL of a 0.4289M pyridine (CH,N) solution with 0.5274M HCI solution at 25…

A: Given,  [C5H5N] = 0.4289 M  Volume of C5H5N in mL = 180.0 mL  [HCl] = 0.5274 M  pKb of C5H5N = 8.77…

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.