Using the Hume Rothery Rules for substitutional solid solution, predict the solubility of the following: Show all your work in details a. H and Ni b. Zn and Fe
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- What is the maximum concentration of Mg++, in formula weights per liter that can exist in a solution which is 0.5F with respect to NH4Cl and 0.1 F with respect to NH34. About 10 mL of concentrated HCl was transferred to a 1-L bottle and diluted to with water. When this solution was used to titrate a sample of pure sodium carbonate weighing 0.3054 g, it took 35.06 mL to reach the methyl red end point. Calculate the molarity of the HCl solution.Calculate the solubility of CuBr (FM 143.45) in water expressed as (a) moles per liter and (b) grams per 100 mL. (This question presumes that Cu1 and Br2 are the only significant soluble species and that species such as CuBr2 andthe ion pair CuBr(aq) are negligible.)
- D. Water Softening 1.For this part of the experiment, watch the video on the link(s) below: https://www.youtube.com/watch?v=jDgSohKVLio Question: Comparison between the relative amount of precipitates for soft vs. hard water.A) Student used 21.03 mL of titrant to reach the endpoint of a titration of 0.1234g sample of Na2CO3. Calculate the ratio of the volume (mL) of titrant used to mass (g) of sample. B) Using the ratio calculated above, calculate the mass of sample necessary to consume exactly 25.00mL of titrant.A 0.4671 g sample containg NaHCO₃(Mwt=84.01mg/mmol) was dissolved and titrated with 0.1067 M HCl requiring 40.72 ml, find the percentage of NaHCO₃, in the sample
- d) the student realizes that the precipitate was not completely dried and claims that as a result, the calculated Na2CO3 molarity is too low. Do you agree or disagree and why? e) after the precipitate forms and is filtered, the liquid is tested to see if it conducts electricity. What would be observed? Explain.0.890 g KIO3 was dissolved to give a 80.00 mL Iodate solution. 35.00 mL aliquot reactedwith the iodide to form triiodide. The liberated triiodide was titrated and consumed 11.65 mL of theS2O32- solution to reach endpoint. Calculate the concentration in molarity of the Na2S2O3solution.How many ml of 0.310M barium nitrate are required to precipitate as barium sulfate all the sulfate ions from 28.0ml of 0.380M aluminum sulfate
- It is desired to neutralize a solution X that contains a mixture of potassium chloride and hydriodic acid. Titration of 11.0 mL X with 0.143 M silver nitrate required 39.2 mL of the latter. The resulting precipitate, containing a mixture of AgCl and AgI, was dried and found to weigh 1.190 g. How much 0.147 M sodium hydroxide should be used to neutralize 11.0 mL solution X?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!Consider the Heat of Solution Practical that was conducted. Temperature (oC) Amount of NaOH ( 0.015M) used to reach end point of titration (ml) 40 42 35 35 30 26 25 23 20 16 Use the data provided above in order to determine the heat of solution. Include any necessary graphs.