Calculate the pH at 25 °C of a 0.30M solution of anilinium chloride (C6H₁NH₂C1). Note that aniline (C6H5NH₂) is a weakbase with a p K₂ of 4.87.Round your answer to 1 decimal place.pH =0XŚolo18Ar

Given, Concentration of anilinium chloride (C6H5NH3Cl) = C = 0.30 M pKb of aniline (C6H5NH2) = 4.87…

alculate the pH at 25 °C of a 0.30M solution of anilinium chloride (CH³NH₂Cl). Note that aniline (CH³NH₂) is a weak ase with a p K₂ of 4.87. ound your answer to 1 decimal place. pH = X BEN olo Ar

alculate the pH at 25 °C of a 0.30M solution of anilinium chloride (CH³NH₂Cl). Note that aniline (CH³NH₂) is a weak ase with a p K₂ of 4.87. ound your answer to 1 decimal place. pH = X BEN olo Ar

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: Consider an aqueous solution that is 0.050 M in H2Se (Ka = 1.29 x 10-4) and 0.075 M in NaHSe. Out…

A: Given, 0.050 M in H2Se 0.075 M in NaHSe

Q: The K, of propanoic acid (C,H,COOH) is 1.34 × 10-³. Calculate the pH of the solution and the…

Q: What is the hydroxide ion concentration

Q: A solution is prepared at 25 °C that is initially 0.45M in methylamine (CH,NH,), a weak base with…

A: Solution- Here we have basic buffer with Kb ; basic ; CH3NH2=0.45 M Acid; CH3NH3Br = 0.49M Kb= 4.4…

Q: OH,O and H,PO OH,PO, and H,PO O HO and H,PO OH,PO, and OH 7) The conjugate base of NH," is OH. O…

A: •This question is based on conjugate acid and base. •So firstly we understand about conjugate acid…

Q: The value of K, for acetylsalicylic acid (aspirin), HC,H704, is 3.00×10-4 Write the equation for the…

A: The equilibrium constant of a chemical reaction is the value of its reaction quotient at chemical…

Q: A weak acid, HA, is a monoprotic acid. A solution that is 0.220 Min HA has a pH of 2.440 at 25°C.…

A: The objective of the question is to find the acid-ionization constant, Ka, for the weak acid HA and…

Q: The value of Ka for phenol (a weak acid) , C,H5OH , is 1.00×10-10 . Write the equation for the…

A: Phenol acts as a weak base that means the hydrogen attached to -OH group in phenol is removed as a…

Q: Tartaric acid is found in many fruits including grapes. Tartaric acid is partly responsible for the…

A: The dissociation of tartaric acid can be represented as: H2C4H4O6+H2O↔HC4H4O6-+H3O+…

Q: Part C Consider the following polyprotic acid solution: 0.135 mol - L H2CO3. Kal = 4.3 x 10-7 Ka2 =…

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

Q: Given the weak acid, boric acid (H3BO3), calculate the pH and pOH of a 4M boric acid solution. Ka =…

Q: A solution is made by dissolving 18.7 g of CH3NH:NO: in 500.0 mL of water. L Does CH.NH:- have any…

A: Given, Mass of CH3NH3NO3 = 18.7 g. Volume of water = 500.0 mL

Q: chloride A solution is prepared at 25 °C that is initially 0.69M in dimethylamine ((CH3)2NH), a weak…

A: First, we need to identify the reaction that is occurring. Dimethylamine ((CH3)2NH) is a weak base,…

Q: What is the pH of a 0.0490 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10-1⁰)?

A: Concentration of HCN solution (c) = 0.0490 M Ka = 4.9×10-10 pH = ?

Q: Aspirin is acetylsalicylic acid, HC,H,O4, which has a K, of 3.0 × 10¬4. Calculate the pH of a…

A: Given information: Mass of acetylsalicylic acid = 0.65 g Volume = 50.0 mL

Q: pH

Q: A solution is prepared at 25 °C that is initially 0.34M in propanoic acid (HC₂H,CO₂), a weak acid…

A: Given data :

Q: 1. The following equilibrium exists when ammonium is dissolved in water: NH4+ (aq) + H2O (l) « H3O+…

Q: What will the concentrations be for a, b, and c? What is the pH of the solution?

A: Concentration = moles/volume.[pyridine] =mol/volume = 0.3mol/1 L = 0.3M.

Q: Calculate the hydronium ion concentration of an aqueous solution of 0.350 M pyridine (a weak base…

Q: What is the pH of a 0.17 M weak acid solution? The KA of the weak acid is 2.1 x 10-5.

A: Given :- Initial concentration of weak acid = 0.17 M Ka for acid = 2.1 × 10-5 To be calculated :-…

Q: A weak acid, HA, is a monoprotic acid. A solution that is 0.220 Min HA has a pH of 2.440 at 25°C.…

A: The objective of this question is to calculate the acid-ionization constant, Ka, for the weak acid…

Q: For the diprotic weak acid H,A, Kal = 3.2 x 10 and Ka2 = 6.3 x 10-9 What is the pH of a 0.0800 M…

A: For H2AKa1 = Ka2 = Concentration of H2A = 0.0800 MWe have to determine the pH of the solution and…

Q: NH3 is a weak base (Kp = 1.8 x 10³) and so the salt NHĄCI acts as a weak acid. What is the pH of a…

A: At Temperature 25°C Kb (NH3) = 1.8 × 10-5 [NH4Cl] = 0.028 M

Q: What is the pH of a 0.16 M solution of methylammonium chloride, CH;NH; Cl? What is the concentration…

Q: Consider a 1.0 L of 0.1 M aqueous solution consisting of weak acid HA, which has K₂ = 3.9 x 10-4, at…

A: HA is a weak acid that is very weakly dissociated to give H+(aq) ions. HCl is a very strong acid…

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

Q: Given that pKa = 3.14 at 25 deg C for HNO2, what is the pH of 0.173 mol L-1 NaNO2(aq) at 25 \deg C?…

A: The objective of the question is to calculate the pH of a 0.173 mol/L NaNO2 solution at 25°C and the…

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: The base protonation constant Kr of trimethylamine ((CH³)²N) is 6.31 × 10¯ b Calculate the pH of a…

Q: pH calculation at the initial point: Calculate the pH of 50.0 mL of 0.250 M oxalic acid (HOOCCOOH)…

Q: The acid dissociation constant K, of acetic acid (HCH3CO,) is 1.8 x 10. Calculate the pH of a 0.52M…

A: Given that : The acid dissociation Ka of acetic acid = 1.8 x 10-5 We have to calculate the pH of a…

Q: Consider an aqueous solution that is 0.050 M in H2Se (Ka = 1.29 x 10-4) and 0.075 M in NaHSe. Out…

A: Given, 0.050 M in H2Se 0.075 M in NaHSe

Q: HX X™ HY Y™ & H30+ Which is the stronger acid? Which is the stronger base? Given the equilibrium…

Q: Consider the following data on some weak acids and weak bases: formula hydrocyanic acid HCN acid…

A: Given,The solutions: Solution pH 0.1 M KCN…

Q: -9 The acid dissociation constant K of hypobromous acid (HBrO) is 2.3 × 109. a Calculate the pH of a…

Q: Part C 0.185 M in HCHO2 and 0.23 M in HC2H3O2

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: What is the pH of a 0.0580 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10-1º)?

Concept explainers

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.

Question

Calculate the pH at 25 °C of a 0.30M solution of anilinium chloride (C6H₁NH₂C1). Note that aniline (C6H5NH₂) is a weak
base with a p K₂ of 4.87.
Round your answer to 1 decimal place.
pH =
0
X
Ś
olo
18
Ar

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1: Introduce question

VIEW

Step 2: Calculate the pH of the solution:

VIEW

Solution

VIEW

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A solution is prepared at 25 °C that is initially 0.37M in nitrous acid (HNO₂), a weak acid with K -4.5 × 10 4, and 0.69M in sodium nitrite (NaNO2). Calculate the pH of the solution. Round your answer to 2 decimal places. a pH X G
1 2 4 Calculate the pH at 25 °C of a 0.59M solution of sodium hypochlorite (NaClO) . Note that hypochlorous acid (HC10) is a weak acid with a p K, of 7.50. Round your answer to 1 decimal place. pH = Software update ready to install. Su Continue O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy C II の

Propanoic acid (CH3CH2COOH) has a Ka of 1.3×10–5.FW(propanoic acid) = 74.08 g/mol; FW(calcium propanoate) = 186.22 g/mol a) At what pH will a solution of propanoic acid and sodium propanoate best resist changes to its pH? How do you know? b) 75 g calcium propanoate Ca(CH3CH2COO)2 is diluted to 150.0 mL with deionized water. 50.0 mL of a 3.0 M propanoic acid solution is added. Determine the equilibrium concentrations of each species and the pH of the resulting solution.
A solution is prepared at 25 °C that is initially 0.15M in propanoic acid (HC₂H-CO₂), a weak acid with K=1.3 × 105, and 0.18M in potassium propanoate (KC₂H,CO₂). Calculate the pH of the solution. Round your answer to 2 decimal places. pH = 0 X S
6. What is the pH of a 0.25 M solution of methylamine hydrochloride (CH3NH3CI)? KÁ for methyl amine (CH3NH2) is 4.4 x 10-4
Calculate the pH at 25 °C of a 0.82M solution of pyridinium chloride (C,H,NHCI). Note that pyridine (C,H,N) is a weak base with a p K, of 8.77. Round your answer to 1 decimal place. pH = |
A solution is prepared at 25 °C that is initially 0.20M in chloroacetic acid (HCH₂CICO₂), a weak acid with K=1.3 x 10³, and 0.34 M in sodium chloroacetate (NaCH₂CICO₂). Calculate the pH of the solution. Round your answer to 2 decimal places. pH = 0 Explanation 81°F Mostly sunny 3 F9 Check $ 4 X с с FS % 5 S 2 1 F6 6 Q Search. F7 & 7 LDL F8 * 8 F9 F10 ( 9 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessi F11 ) 0 *+ F12 JE PrtSc + Insert = Delete Backspace 4) J ►/11 Num
HCN is a weak acid (K, = 6.20 × 10-0), so the salt, KCN, acts as a weak base. What is the pH of a solution that is 0.0405 M in KCN at 25 °C? pH =
What is the concentration of hydroxide ion in a 0.76 M aqueous solution of hydroxylamine, NH2OH? (Assume the value of Kw is 1.0 10-14.) what is M ? What is the pH ?
What is the concentration of H3O+ in a solution that is 0.0600 M Hypochlorous acid (HClO)? What is the pH? To solve this problem: Write the acid dissociation equilibrium for HClO Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, ClO- and HClO at equilibrium, in terms of x. Decide if x can be neglected. You may neglect x if the initial concentration of the HClO is greater than 100 times the Ka. You will need the value of Ka. Look it up on the chart (p 4 of packet) Solve for x Find the pH The pH of a 0.0200 M solution of an unknown acid is 2.56. What is the Ka of this acid? To solve this problem: Write the acid dissociation equilibrium for the generic aicd “HA” Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, A- and HA at equilibrium, in terms of x. What is x? Can you find it…
What is the pH of a 0.652 M solution of hydroxylammonium, a weak acid with a K, of 1.1 x 10-6? Oa. 0.19 Ob. 3.07 Ос. 7.2 х 10-7 Od. 5.96 Oe. 6.14
3.