llء ا31۸:۲ ص 0 04العربية -الإنجليزية-الإنجليزيةQ2// 1000 ml of o.1Mhydrochloric acid wereadded to 1000 ml of o.IMammonium hydroxide,ammonium chloride salt wasformed. Calculate the pHfor the salt solution. Kb-1.8x10-5تحويل الصوت إلى نصمحادثةكاميراالعربيةتمت إضافة 0 0 10 / / Q2 مل منحمض الهيدروكلوريك 1.o مولارإلى 0 100 مل من هیدروكسیدالأمونيوم o.IM ، وتم تكوین ملحكلوريد الأمونيوم. احسب الرقمالهيدروجيني لمحلول الملح. كيلوبایت 1.8 5-10x

Since we know that pH + pOH = 14 and also pOH = pkb + log[salt]/ [base]

Answered: الإنجليزية Q2// 1000 ml of o.1M…

الإنجليزية Q2// 1000 ml of o.1M hydrochloric acid were added to 1000 ml of o.IM ammonium hydroxide, ammonium chloride salt was formed. Calculate the pH for the salt solution. Kb-1.8 x10-5

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: Determine the pH of the resulting solution by mixing 0.36 M of sodium formate (HCOONa) of 20.0 mL…

A: As 0.36M of sodium formate of 20.0 ml is mixed with 0.18 M of HCl of 40.0 mL, thus equivalence point…

Q: 22.5 mL of a 0.200 M HBr solution was added to a 50.00 mL sample of 0.250 M Sodium benzoate…

A: Given that: 50.00 ML of 0.250m NaC7H5O2 Molarity =molesvolume moles of…

Q: Which weak acid would be best to use when preparing a buffer solution with a pH of 9.50? an acid…

A: A buffer is a solution which resists any change in pH on adding a small amount of acid or base.It is…

Q: Calculate the pH of a solution prepared by adding 30.0 mLs of 0.20 M HCl to 50.0 mLs of 0.10 M…

A: Given: Concentration of HCl = 0.20 M Volume of HCl solution = 30.0 mL = 0.030 L…

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: 1. a. What is the pH of a solution prepared by adding 25.0 mL of 0.10 M acetic acid (Ka = 1.8 x…

Q: A chemist titrates 140.0 mL of a 0.4198M dimethylamine ((CH3)2NH) pK, of dimethylamine is 3.27.…

Q: Calculate the pH of a solution made by mixing 20.0 mL of a 0.100M methanoic acid (CHOOH) with 80.0…

Q: A solution is made by combining 12.7 mL of 16.5 mol L-1 benzoic acid (Ka = 6.3 x 10-5) with 5.39 g…

A: Given: Volume of benzoic acid = 12.7 mL = 0.0127LMolarity of benzoic acid = 16.5 mol/LTherefore,…

Q: To determine the identity of a compound, a student dissolved 0.72 g of the compound in enough water…

A: First we need to check the initial solution by initial value of pH. Then nature of titrant which is…

Q: Calculate the pH of a solution formed by mixing 150.0 mL of 0.10 M HC7H502 with 100.0 mL of 0.30 M…

Q: Q1// A buffer solution prepared by adding adequate amount of Acetic acid and Sodium acetate to…

A: Firstly we will calculate pH of buffer solution CH3COOH - CH3COONa CH3COOH (aq) + H2O (l)⇌H3O+…

Q: olution is made by mixing 185 mL of 0.100 M formic acid (Ka = 1.7 x 10-4 ) with 190. mL of 0.100 M…

Q: 4

A: For the formation of cyclic acetals , you always need a carbonyl compound (ketone/aldehyde) and…

Q: Which of the following acid/base conjugate pairs could you use to make a buffer solution with a pH…

Q: Calculate the pH for each of the cases in the titration of 25.0 mL of 0.170 M pyridine, C, H, N(aq)…

A: we need to calculate the pH of the given solutions

Q: Calculate the pH of the solution after 500 mL of the titrant have been added. Express your answer to…

A: The concentration of the acetic acid is Ca = 0.010 M,The volume of the the acetic acid is Va = 500…

Q: Calculate the pH of a solution formed by mixing 500.0 mL of 0.075 M CH3NH3Cl with 200.0 mL of 0.10 M…

A: Given: Volume of CH3NH3Cl = 500 mLMolarity of CH3NH3Cl = 0.075 MVolume of CH3NH2 = 200 mLMolarity of…

Q: A 1000.0 mL solution contains 0.150 M NaCIO and 0.200 M HCIO. What is the pH of this solution before…

A: pH = pKa + log[salt]/[acid] pKa = -logKa

Q: Calculate the pH at the equivalence point of 25.0 mL solution of ascorbic acid, titrated with 45.3…

Q: You mix 100.0 mL of 0.20 M NaCH3COO with 20.00 mL of 0.200 M HCl. Calculate the pH of the mixture.…

A: Ka of CH3COOH = 1.8×10-5 Calculation of pKa of CH3COOH:

Q: Calculate the pH of the following mixture 500 ml 0.35 M HCl + 500 ml 0.25 M CH3CH2NH2

Q: A chemist titrates 190.0 mL of a 0.5359 M hydrobromic acid (HBr) solution with 0.2938M KOH solution…

Q: (a) Devise a cell for evaluating the solubility product of PbSO4 (PbSO, Pb²+SO). Calculate the…

A: According to the question we have a reaction of cell, PbSO4 + 2e- ⇔Pb + SO42- The temperature is…

Q: Select the mixture which is capable of tolerating the addition of a strong acid without altering the…

Q: A chemist titrates 190.0 mL of a 0.3300M methylamine (CH3NH2) solution with 0.2028M HBr solution at…

A: Given:Volume of methylamine solution = 190.0 mL (0.190 L)Concentration of methylamine: 0.3300…

Q: The equation Hln = H + In means? آختر احدى الدجابات A. The medium is acidic or basic B. Which form…

A: Hln = H+ + ln- If acid is added then according to Le-Chatelier’s principle, the reaction will…

Q: A chemist titrates 60.0mL of a 0.0558M butanoic acid HC_3H_7CO_2 solution with 0.5376M NaOH solution…

Concept explainers

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.

Question

llء ا31
۸:۲ ص 0 04
العربية -
الإنجليزية-
الإنجليزية
Q2// 1000 ml of o.1M
hydrochloric acid were
added to 1000 ml of o.IM
ammonium hydroxide,
ammonium chloride salt was
formed. Calculate the pH
for the salt solution. Kb-1.8
x10-5
تحويل الصوت إلى نص
محادثة
كاميرا
العربية
تمت إضافة 0 0 10 / / Q2 مل من
حمض الهيدروكلوريك 1.o مولار
إلى 0 100 مل من هیدروكسید
الأمونيوم o.IM ، وتم تكوین ملح
كلوريد الأمونيوم. احسب الرقم
الهيدروجيني لمحلول الملح. كيلو
بایت 1.8 5-10x

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

VIEW

Step 2

VIEW

Step by step

Solved in 2 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

18
What is the pH of a solution created by mixing 25.00 mL of 0.10 M formic acid and 25.00 mL of 0.10 M sodium format? Ka of formic acid is 1.8 X 10-4 -1.8 X 10-4 -3.74 -4.74 -1.00
An analytical chemist is titrating 154.7mL of a 0.2900M solution of dimethylamine CH32NH with a 0.3400M solution of HNO3. The pKb of dimethylamine is 3.27 . Calculate the pH of the base solution after the chemist has added 155.7mL of the HNO3 solution to it. Round your answer to 2 decimal places.
Please don't provide handwriting solution
What is the pH of a solution which is mixture made with 10 mL 0.30M in ammonia NH3 and 30mL 0.1M of HCl? Kb for ammonia NH3 = 1.8 x10-5
Calculate the pH of the following mixture 500 ml 0.35 M HF + 500 ml 0.25 M KOH
We add 10mL of 0.1M NaOH to 100mL of 0.1M CH3COOH/ 0.1M CH3COO^-. (Ka = 1.8 x10 ^-5). Using the Henderson-Hasselbach equation, pH=pKa + log [A-]/[HA] a) before the addition of NaOH b) after the addition of NaOH
K, for hypochlorous acid, HCIO, is 3.0×10-8, Calculate the pH after 10.0, 20.0, 30.0, and 40.0 mL of 0.100 M NaOH have been added to 40.0 mL of 0.100 M HC10.
What is the pH of the solution that results from mixing 25 mL of 2.20×10-2 M NH3 and 25 mL of 2.20×10-2 M HCl? Ka (NH4+) = 5.60×10-10 pH =
An analytical chemist is titrating 149.0mL of a 0.2200M solution of piperidine C5H10NH with a 0.3200M solution of HNO3 . The pKb of piperidine is 2.89 .Calculate the pH of the base solution after the chemist has added 113.4mL of the HNO3 solution to it. Round your answer to 2 decimal places.
If a 0.552M HCl caq) solution is used by a scientist to titrate 10.00mL of a weak base, based curve (shown below), what base? write your the titration the concentration of the auswer with 4 decitual places. pH Curve OM is 12 10 8 6 4 2 0 5:0 2 1.5 n 3 3.5 A Volume of Titrant / mL 7.5 8 8.5
What is the pH of a solution prepared by mixing 20.0 mL of 0.50 M NaOH and 35.0 mL of 0.50 benzoic acid solution? (Benzoic acid is monoprotic with a Ka of 6.5 x 10-5.)