Consider the following reaction:Enter the complete ionic equation for this reaction.Express your answer as a complete ionic equation. Identify all of the phases in your answer.esc| ΑΣΦ 1SubmitDA chemical reaction does not occur for this question.Part B Complete previous part(s)Provide FeedbackMother to Son &.pdf!1Request AnswerQA2optionN239WS3XHcommand?80ED$4CaFARLLF%LO2HBr(aq) + Ca(OH)2 (aq) → 2H₂O(1) + CaBr₂(aq)5FSVT.MacBook Air6GFOYB&N7HU+008NJD--11FO(109TbibMFOK)OO<2

An aqueous solution of hydrogen bromide reacts with an aqueous solution of calcium hydroxide to form…

Consider the following reaction: Enter the complete ionic equation for this reaction. Express your answer as a complete lonic equation. Identify all of the phases in your answer. ΑΣΦ A chemical reaction does not occur for this question. Submit Request Answer Part B Complete previous part(s) ? Provide Feedback 2HBr(aq) + Ca(OH)2 (aq) → 2H₂O(1) + CaBr₂ (aq)

Consider the following reaction: Enter the complete ionic equation for this reaction. Express your answer as a complete lonic equation. Identify all of the phases in your answer. ΑΣΦ A chemical reaction does not occur for this question. Submit Request Answer Part B Complete previous part(s) ? Provide Feedback 2HBr(aq) + Ca(OH)2 (aq) → 2H₂O(1) + CaBr₂ (aq)

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter7: Statistical Data Treatment And Evaluation

Section: Chapter Questions

Problem 7.10QAP

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Table 2. Gibbs Free Energies of formation (kJ), ∆G°f, for Ions in 1M Solution and Ionic Solids Cations Cl--131.228 I--51.57 NO3--108.74 SO4-2-744.53 Ag+77.107 AgCl -109.789 -66.19 -33.41 -618.41 Calculated values of ∆G°rxn and the ∆Grxn of each box, Predicted results (ppt or no ppt).Observations (Rxn or No Rxn). S or support and R for Refute Cations Cl- I- NO3- SO4-2 Ag+ Ba+2
By the use of Henderson Hasselbalch equation; pH = pKa + log{[acetate ion]/[acetic acid]} 4.5 = 4.75 + log{[0.10 M]/[acetic acid]} -0.25 = log{[0.10 M]/[acetic acid]} [Acetic acid] = 0.10 M/ 10-0.25 [Acetic acid] = 0.10 M/0.56 [Acetic acid] = 0.1786 M Moles of sodium acetate dissolved in 250 mL buffer solution = 0.10 M× (250mL/1000mL) × 1L = 0.025 mol Weight (w) of sodium acetate (purity 100%) dissolved to prepare 250 mL of solution with buffer concentration of 0.10 M is calculate as follow; w100% = 0.025 mol × 82.0343 g/mol = 2.051 g Weight (w) of sodium acetate (purity 99%) is calculate as follow; w99% = 2.051 g× (100/99) = 2.072 g What was the volume of 6.12 M acetic acid HC2H3O2 needed to prepare the 250 mL acetic acid/acetate ion buffer solution required in this part? Show your calculations.
Consider the following heterogeneous reaction where a solid product B is formed:` `A (g) ↔ B (s) + 2 D (g)a) How many phases are present?b) What is the maximum amount of solid product B that can be produced for every mole of A fed to the reactor if the reactor is operating at 1000 K and 1 bar? Data: K = 2.04 at 1000 K.
The student then determined ΔH neutralization for the reaction of sodium hydroxide and acetic acid, using the procedure described in this module. The student added 100.0 mL of 0.8500M NaOH to 100.0 mL of 0.8404M acetic acid. Prior to and following the mixing of the acid and base solutions, the following temperature-time data were collected. g) Identify the limiting reagent and briefly explain why it is limiting. h) Find ΔH neutralization for the reaction.
Ca2+ and CO32- are dissolved in a beaker of sea water at 298 K, resulting in formation of a CaCO3precipitate:Ca2+ (aq) + CO32- (aq) ⇋ CaCO3 (s) ΔH0 = 13.44 kJ mol-1, ΔS0 = -120 J mol-1 K-1(i) Determine the direction of spontaneity under standard state conditions.(ii) Determine ΔG when [Ca2+] = 0.01 mol dm-3 and [CO32-] = 45 μmol dm-3. The activity coefficients of Ca2+ and CO32- in sea water are 0.28 and 0.21 respectively.
KMnO4 and Na2C2O4 solutions were used in the reactions that took place in a back titration to determine the amount of H2O2 in a sample. Calculate the concentration of H2O2 in the sample (w / v) as% by making appropriate assumptions for the volumes and normality of all these solutions.
The pressure dependence of G is quite different for gases and condensed phases. Calculate ΔGm for the process (C,solid,graphite,1bar,298.15K)→(C,solid,graphite,300.bar,298.15K) The density for graphite is 2250 kg⋅m−3 Calculate ΔGm for the process (He,g,1bar,298.15K)→(He,g,300.bar,298.15K)
Note: Express % strength with 4 decimal places. For ratio strength, state the volume only% Astelin nasal spray contains 0.1% azelastine hydrochloride and 125 mcg/mL of benzalkonium chloride as a preservative. A container is capable of delivering 200 metered sprays of 0.137 mL each. The percent concentration of benzalkonium chloride in the preparation is _______%, which is equivalent to a ratio strength of 1 in _____ w/v.
The assumptions about the virtual process state diagrams of metals A and B similar to the lead-tin system in Figure 9.8 are as follows. (1)The α phase and β phase exist at both ends of A and B. (2) The process composition is 36 wt% A to 64 wt% B. (3) The composition of β phase at the process temperature is 88 wt% A to 12 wt% B. Find the composition of an alloy in which the weight fraction of invitation β and total β is 0.367 and 0.768, respectively.
a)Write a balanced equation for the dissolution of PbBr2. Express your answer as a chemical equation. Identify all of the phases in your answer. b) Write a balanced equation for the dissolution of Ag2CrO4. Express your answer as a chemical equation. Identify all of the phases in your answer. c)Write an expression for Ksp for the dissolution of Ag2CrO4.
For the reaction pictured, the experimental enthalpy is -41.3 ± 1.3 kJ mol-1. When using the Gaussian command line # B3LYP/6-31G(d) opt freq int=grid=ultrafine, the enthalpy was -40.1, but when using the Gaussian command line # MP2/cc-pVTZ scf=tight, the enthalpy was -42.4. What would cause one method to be more accuarate than the other? Thank you :)