Complete the balanced dissociation equation for the compound below in aqueous solution. If the compound does not dissociate, write NR after the reaction arrow. NaBr (s) →
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- Q2- Give scientific explanation with equations for the following: I+ Despite of precipitant agent of both of cations of groups IV and I is sulfide ion. but they are separated. 2. A mixture of ammonium hydroxide and ammonium chioride s a source of hydroxide ion of ‘group three. 3- Cations of group Il is divided into sub groups a and b.A 0.217 g sample of HgO (molar mass = 217 g/mol) reacts with excess iodide ions according to the reaction show below. Titration of the resulting sample solution requires how many moles of 0.10 M KI to reach the equivalence point? Assume complete reaction. HgO + 4 I- + H2O HgI42- + 2 -OHIf a titration net volume for the standardization should be 23.50 mL and a student accidentally one drop past the endpoint (~0.05 mL), will the calculated NaOH concentration (M) be higher or lower than the true value of that solution’s concentration? Explain briefly.
- When all of the following are mixed together in a beaker, what is the molar concentration of the SCN- ion in the solution just after mixing but before any reaction takes place? 10.00 mL of 2.00 x 10-3 M Fe(NO3)3 4.00 mL of 2.00 x 10-3 M KSCN 4.00 mL of 0.50 M HNO3 answer is between 0.004 and 0.005, please explain how with steps.The reaction of KOH with HNO2 is presented by the unbalanced chemical reaction below: ___ KOH(aq)+ ___ HNO3 (aq)---> ___ KNO3 (aq)+ ___ H2O(l)Calculate the molar concentration of Nitric acid (HNO2) when 40.5 mL of 0.674 M KOH is required to quench 101.0 mL of Nitric acid over phenolphthalein indicator.Is it possible, upon precipitation of the third class ions, to add H2S first, then NH4OH and NH4Cl? And why
- I would really appreciate some help in confirming a value computed in a prelab problem to be used in a lab for analytical chemistry! We're working on redox reactions and are looking at the reaction: Fe2+ + K2Cr2O7 + H+ = Fe3+ + K+ + Cr3+ + H2O The final questions asks, "calculate the amount of unknown sample needed to achieve about a 25.00 mL titration volume of 0.01600 M K2Cr2O7 if the %Fe of the unknown is approximately 8%. Make sure to use the coefficients from the balanced reaction" I have found the balanced equation; however, I was hoping to be able to confirm my values! Thank you in advance!The overall formation constant for HgI42- is 1.0x1030. That is, 1.0x1030 = [HgI42-] / [Hg2+] [I-]4 What is the concentration of Hg2+ in 400.0 mL of a solution that was originally 0.016 M Hg2+ and 0.72 M I-? The reaction is Hg2+ (aq) + 4I- (aq) <----> HgI42- (aq) [Hg2+] = ____________ MWhat hydroxide concentration is required to a. initiate precipitation of Al3+ from a 2.50 X 10-2 M solution of Al2(S04)3?b. lower the AI3+ concentration in the foregoing solution to 2.00 X 10-7 M?
- Compute the solubility of Mg(OH)2 in a buffer solution at pH=10.42. The solubility product of magnesium hydroxide is 1.2E-11Include at least 3 significant figures in your answer.In solutions 1-4 you are adding successively larger volumes of 0.00200 M SCN- to the Fe3+ solution and diluting to 10.00 mL. Calculate the final diluted molarity of SCN- in solution #1. 3 sig figs (Calculate the same thing for the solutions 2-4 and enter the results in table 3 as [SCN-] pre-equilibrium.)v. What is pH? Calculate the pH for 0.0001N NH4OH solution of 100mL volume. The pKb value for NH4OH at 25oC is 1.76 x 10-5.