ulate the molar AH for each trial. Show work neatly for credit. molar AH (kJ/mol) -81.3kJ/mol Trial -467.0K5/ml -473.6 kJ/mol Trial 2 Trial 3 2. Write a balanced equation for the two reactions, Mg + HCI, and MgO with HCI. + H₂ (9) + 2HCl (aa) MgCl 2 (aq) Mg (s) MgO (s) + 2HCl caq) -> Mg Cl₂ caq) + H20) 3. Calculate the average molar AH for each of the reactions. AH = >H Trial + DH trial 2 + AH Trial3 3 AH -81.3 + (-467.0) + (-473.6) 3 4. Use Hess's Law to determine the AH for the reaction: Mg(s) + 1/202(g) MgO (s) 2-340.63kJ/mol You will need to use the experimentally determined AH's and the standard heat of formation of water (1) to determine this. Show your work neatly for credit. 205.0 2x83.5 5. Calculate the % error of your AH as compared to the textbook value for the heat of formation of MgO. Show your work neatly for credit.

What is the pH of a saturated solution of Ca(OH)₂? Ca(OH)₂ (s) Ca²+ (aq) + 2 OH- (aq) село N O +25 25 initial -§. pH of Hydroxides - Example ех сего +s S Ksp= [Ca²+] [OH-]²= (5)(25)²=453 5= 33.7x² 3.7 хо S (OH) = 25 = 0.019487 M = 0.009713 M Ksp = 3.7 x 10-6 [++] = 10²] -14 pH=12.29 -= 5-1316x180-13 [он) pH = -log (H+) =-loğl pH = 12.2897

Please help with this homework question. Thank you!

Consider the reaction of a 20.0 mL of 0.220 M CsH5NHCI (Ka = 5.9 x 10-6) with 12.0 mL of 0.215 M CSOH. a) Write the net ionic equation for the reaction that takes place. Be sure to include the proper phases for all species within the reaction. b) What quantity in moles of CsHsNH+ would be present at the start of the titration? c) What quantity in moles of OH- would be present if 12.0 mL of OH- were added? d) What species would be left in the beaker after the reaction goes to completion?

ALL INFORMATION NEEDED IS PROVIDED, I NEED FIRST QUESTIONS ANSWERED FIRST BEFORE OTHERS CAN BE ANSWEREDRate = -(Delta[RCl])/Delta t andln[RCl]t=-k*t+ln[RCl]0 < [R-Cl]-time equation Test tube A = 0.30 of 0.10M NaOH(aq), 6.70ml DI H2O & 1 drop of bromophenol bue Test Tube B = 3.00M of 0.10M R-CL in acetone. Mix together in 3 water baths Bath A Trial 1= 20C, 53.6s Trial 2= 20C, 49s for color to changeBath B Trial 1= 32C, 18s Trail 2= 32C, 20s Bath C Trial 1= 10C, 204s Trial B= 10C, 200s average out both trials for each bathcolor change happens after 10% of R-Cl has reacted so In terms of R-Cl this means that 10% of the R-Cl has reacted and ____ of the R-Cl is left Q1. at the time of the color change [R-Cl]t=____[R-Cl]o (Fill in the blank) Q4. Substitute the value of [R-Cl]t into appropriate equation listed above and solve for k in terms of [R-Cl] and t. Q5. Use average time for each temp and determine the value of k (with units) at each temperature Q6. Rearrange the Arrhenius…

Complete the chart using the information provided in the second image. Show setup for the calculation of the molarity of the HCI for Trial 1 and also show the setup for the Calculation of the percent HCI in the solution.

Complete solution -Buffer Preparation-

Could someone help me answer these questions? I am unsure on how to go about this.

-5 A solution is prepared at 25 °C that is initially 0.051M in acetic acid (HCH3CO₂), a weak acid with K = 1.8 × 10 (NaCH3CO₂). Calculate the pH of the solution. Round your answer to 2 decimal places. a pH = 【 X Ś I and 0.033 M in sodium acetate

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