Upload all your work and calculations here

What is the molarity of the hydrochloric acid if the student used 35.25 mL of 0.1175M standard solution of NaOH to titrate 20.00 mL of acid to the endpoint?

Consider the data table below to calculate the enthalpy of reaction for the neutralization of nitric acid by barium hydroxide.   Volume   of 1.021MHNO3,  mL 50.00 60.00 70.00 80.00 90.00 100.0 Volume of 0.572MSr(OH)2, mL 100.0 90.00 80.00 70.00 60.00 50.00 Change of temperature, oC 4.54 5.45 6.36 7.27 6.54 5.46 Analyze the Data Table to find the highest temperature and answer the following questions. Consider the density of the solutions to be the same as water, 1.00 g/mL, both before and after mixing, and the heat capacity is the same as for water, 4.18J/oCg.  Since your calculators may give you slightly different numbers, pick the closest answer. The highest temperature change in oC[temp]  Number of moles of acid  at the highest temperature (at stoichiometric ratio)[molesA] Number of moles of the base  at the highest temperature (at stoichiometric ratio)[molesB] Mole fraction of acid and mole fraction of base at the highest temperature (at stoichiometric ratio)[MF] Stoichiometric mole ratio for the reaction: moles acid/moles base, calculated [MR] Stoichiometric mole ratio for the reaction: moles acid/moles base, rounded to the whole number[MR2] Heat absorbed by the solution in the calorimeter, J[q] Heat in kJ produced by the reaction between solutions of acid and base in the calorimeter[q2] Heat of reaction in kJ per number of moles of base[H] Thermochemical equation and Enthalpy of the neutralization reaction (Hint: Enthalpy is per number of moles of water)[Eq] Show work for Partial Credit, take a picture of your work, save it to your Canvas files, and upload your answer in the Work and Calculations assignment provided.

The completion of acid-base titration is represented by the end-point and equivalence point. What is the end-point?

Balance the following reaction and determine the coefficient for water. __P2O5(g) +  __H2O(l) →  __H3PO4(aq)

  Apply the Hess’s Law and use the Data table below to calculate the ΔH°rxn, in kJ, for: Sr(OH)2(s) + 2HNO3aq) => Sr(NO3)2(aq) + 2H2O(l) Show work for Partial Credit: take a picture of your work, save it to your Canvas files, and upload your answer in the Work and Calculations assignment provided. Substance  ΔHf° (kJ mol–1) Sr(OH)2(aq) -1007.3 HNO3(aq) -206.63 Sr(NO3)2(aq) -962.32 H2O (l) -285.83  

A sample of gas occupies a volume of 160.0 L at 155° What will be the volume of gas in mL when the temperature drops to 55° C at the same pressure?

Write and balance the equation and determine the mole ratio of reactants. Use this information to answer the following questions: How many moles of NaOH are present in 255 mL of 2.7471M solution?[A] How many moles of H3PO4 are needed to completely neutralize this base?[B]

1. The following table was filled by the student during the measuring of the absorbance of a 100 mM solution of Ni2+ ion. Wavelength Absorbed (nm) Color Absorbed Color Observed Absorbance of solution 410 Violet Yellow-Green 0.23 430 Blue-Violet Yellow 0.52 480 Blue Orange 0.07 500 Blue-Green Red 0.03 530 Green Purple 0.01 560 Yellow-Green Violet 0.01 580 Yellow Blue-Violet 0.01 610 Orange Blue 0.03 680 Red Blue-Green 0.16 720 Red-Purple Green 0.19 Select a correct wavelength to measure the absorbance of nickel-containing solutions and justify your answer (4pts):           2. The following calibration table was built in order to calibrate the colorimeter: Test tube # Concentration of Ni2+ ions, M Absorbance Blank 0.000 0.00 Test tube 1 0.020 0.12 Test tube 2 0.040 0.20 Test tube 3 0.060 0.34 Test tube 4 0.080 0.44 Test tube 5 0.100 0.51 Test tube 6 0.120 0.62 Test tube 7 0.140 0.70 Test tube 8 0.160 0.80 Test tube 9 0.180 0.96 Test tube 10 0.200 1.10 Report the equation of the trendline in terms of Absorbance, Molarity and molar absorptivity (you do not need to show the graph) and the value of R2(6pts, report your answer):   3. The 15.0 g sample of Zn-Ni alloy was dissolved in the nitric acid and diluted to 250.0 mL. The measured absorbance of the solution was 0.75. Use the calibration curve equation to calculate and report:Molarity of the solution (3 pts, report your answer): %Ni in the alloy (3 pts, report your answer): Show work for Credit: take a picture of your work, save it to your Canvas files, and upload your answer in the Work and Calculations assignment provided.

Consider the following reaction: NaCl(aq) + AgNO3(aq) => AgCl(s) + NaNO3(aq)  According to the reaction stoichiometry how many number of moles of silver chloride will form if 3.0 moles of sodium chloride react with the excess of silver nitrate? of moles of AgNO3, silver nitrate?