Certainly! Here is the transcription for educational purposes:---2. Write net ionic equations for the hydrolysis of the given ions with H₂O.a. NH₃: ________________________________________________________b. HBr: ________________________________________________________c. S²⁻: ________________________________________________________d. Fe(H₂O)₆³⁺: ________________________________________________________---In this task, students are asked to provide the net ionic equations showing the hydrolysis reactions of the specified ions with water. Each segment provides a space for writing the specific chemical reaction involving the ion listed.

Hydrolysis is the chemical process of the addition of water molecules to a chemical substance, in general. However, this process is also used to break down the compounds into their ionic constituents.2. The net ionic equations for the hydrolysis of the following ions with H2O (water) are as follows: a. NH3 (ammonia) + H2O → NH4+ (ammonium ion) + OH- (Hydroxyl radical) → NH4OH (Ammonium hydroxide) Ammonia in presence of water first splits into ammonium ion with a positive charge and hydroxide radical with a negative charge which further adds up to form ammonium hydroxide. b. HBr (Hydrogen Bromide) + H2O → H3O+ (hydronium ion) +Br– (Bromine ion) Hydrogen Bromide in presence of water splits into bromine ion with a negative charge and hydronium ion with a positive charge. c. S2- (Sulfide ion) + H2O → H2S (Hydrogen Sulfide) + OH- (Hydroxyl radical) Sulfide ion in presence of water first forms an intermediate compound, that is, HS and hydroxyl radical which ultimately combines with more water to form hydrogen sulfide. d. Fe(H2O)6+3 (Hexa-aqua ferrous) + H2O → [Fe(H2O)5(OH)]+2 + H3O+ Hexa-aqua ferrous is a coordination compound containing 6 moles of water and iron in its +3 oxidation state. Upon addition of water first forms penta-aqua hydroxo ferrous with the oxidation state is +2 in iron and hydronium ion.

Answered: 2. Write net ionic equations for the…

Science

Chemistry

2. Write net ionic equations for the hydrolysis of the given ions with H2O. a. NH3: b. HBr: c. S2- d. Fe(H2O)6+3

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

Similar questions

3. Predict whether the following salts, which are insoluble in water, would be dissolved by addition of a strong acid, such as HNO3. If solution occurs, write the net ionic equation for the reaction. Salt Does It Dissolve? Equation for Reaction or Reason for No Action a) MgCO3 b) AgCl c) Ca3(PO4)2 d) ZnS e) BaSO4
A buffer solution is composed of 1.324 g of KH,PO4 and 4.362 g of Naz HPO4. (K, for dihydrogen phosphate ion is 6.2 × 10-8.) a. What is the pH of the buffer solution? pH = b. What mass of KH;PO4 must be added to decrease the buffer solution pH by 0.10 unit from the value calculated in part a? Mass =
1. A water has pH = 8.8 and an alkalinity of 3.2 meq/L. Estimate the concentrations of: a. H₂CO3* b. HCO3 C. CO3² d. Calculate the maximum concentration of calcium ion (Ca2+) that can exist in this water sample without precipitating CaCO3(S)
Jj.107.
O D. HBRO3 OE HF QUESTION 13 Calculate the solubility of silver oxalate, Ag2C204, in 0.05M Na C,04 solution. KED = 1.0 x 10 11 Write answer in scientific notation to two significant figures. When writing scientific notation use "E". For example, 0.0003 would be answer QUESTION 14 Which of the following, if any, would NOT be a buffer solution? OA. all are buffer solutions O B. 0.3M C6H5COOH/0.2M C6H5COONA OC.0.2M HI/0.4M NaF O D.0.1M NAHCO3 /0.1M Na cO, E.0.2M HCI0/0.4M KOH Type here to search 耳 e
8. A student conducts an acid-base titration to investigate the change in pH during a reaction between hydrochloric acid and ammonia solution. a. Name a piece of equipment that could be used to provide an accurate measurement of pH during the titration and explain how it would be calibrated. The student transfers 50cm3 of 1.0moldm3 ammonia solution acid into a beaker. During the titration the student adds 50cm3 1.00moldm³ hydrochloric acid from a burette into the beaker and records the pH throughout. b. Sketch the pH curve produced during this titration.
35
What concentration ratio of NH3 to NH4Cl is necessary to get a buffer solution with a pOH of 5.3? Kb = 1.8x10-5 a. 1:5.1 b. 1:3.6 c. 1:1.7 d. 1.9:1 e. 3.3:1