k. What is the hydroxide concentration of a substance with a pOH of 8.5? 5. Write the dissociation equation for each of the following: l. sodium sulfate m. magnesium hydroxide n. calcium bromide. 6. Draw the Lewis structure for CH3Cl.
It is called the heat of solution of solid NaOH. From our calculation it known that ∆H3 is -58.6 kJ/mol. When ionic solid dissolves in water, heat was librated. Reaction 1: Dissolving solid sodium hydroxide in water. NaOH(s) ---> Na+(aq) + OH-(aq) + heat Reaction 2: Reaction of sodium hydroxide solution with dilute hydrochloric acid.
Lab Report Example Lab 16-1: How much calcium carbonate is in an eggshell? Elizabeth Shanor April 25, 2005 Purpose: Eggshells are composed in part of calcium carbonate. Calcium carbonate reacts with an acid to produce carbon dioxide, water, and a salt. The calcium carbonate in the sample eggshell will be determined by means of reaction with a carefully measured quantity of hydrochloric acid present in excess. The excess acid will be reacted with sodium hydroxide to determine how much acid remains.
The following steps were performed to create the ionic reaction. 2 drops of Sodium Phosphate, Na3PO4?12H2O solution were placed into the five vertical wells under column number 1. Next, 2 drops of Sodium Iodide, Nal solution were placed into the five vertical wells under 2. Next, 2 drops of Sodium Sulfate, Na2SO4 solution into five vertical wells under 3. Next, 2 drops of Sodium Chloride, NaCl solution were placed into the five vertical wells under 4.
2Al + Fe2O3 ( Al2O3 + 2Fe (26.98) ( 159.7) (101.96) 124 601 80 b. Al c. 234.3 d. 234 e. 34.1% 1c. A strip of zinc metal with a mass of 2.0g undergoes single displacement reaction with an aqueous solution containing 2.5g of silver(I) nitrate A. Write a balance equation for the above reaction B. Which of the 2 reactants is the limiting reagent? C. Calculate the mass of zinc (II) nitrate formed D. How much excess reagent is left at the end of the reaction?
The total acid neutralizing capacity of a soda ash sample, its alkalinity value, can be stated in terms of percent sodium carbonate. In doing so, any sodium hydrogen carbonate present in the sample is converted to its equivalent neutralizing capacity in terms of sodium carbonate. That is, a 100% NaHCO3 sample is represented as a 50% Na2CO3 sample in terms of its acid neutralization capacity. It is not uncommon to group compounds of similar behavior together and state the composition in terms of one of them. For example, the potassium content of fertilizer is stated as percent K2O, although the potassium compounds actually present may be phosphates, nitrates or carbonates.
Who is right, John or Anna? Explain your answer. 3 When 200 g of calcium nitrate, Ca(NO3)2.2H2O is heated at 120ºC the mass decreases by 36 g. (a) Why does the mass decrease? (b) How much calcium nitrate is left after heating? 4 Calculate the molar mass of these compounds: (relative atomic masses: H = 1; N = 14; O = 16; S = 32; Cu = 64; Br = 80; Pb = 207) (a) copper nitrate, Ca(NO3)2 (b) lead bromate, Pb(BrO3)2 (c) ammonium sulfate, (NH4)2SO4 5 The equation for the complete combustion of methane is shown below.
At 50C our results indicated a solubility of 89 g/100mL of H2O which was close to the known solubility of 80 g/100mL. Introduction: When a salt, such as potassium nitrate or sodium chloride, is placed in water a dissolving reaction will occur. At first, the positive and negative ions of the salt compound are only attracted to each other. In order for the salt to dissolve, these bonds must be broken so that the ions disassociate from each other. In the water molecules, hydrogen is slightly positive and oxygen slightly negative so they are attracted to ions of the opposite charge, known as dipole attraction.
Using the equilibrium constant from above, calculate the equilibrium concentrations of all the compounds in the reaction if 1.000M acetic acid is reacted with 2.000M ethyl alcohol. Assume the temperature remains constant. 3. The density of a solution of 3.00M HCl solution is 1.05 g/ml. Calculate the mass of water present in 5.00 ml of the solution.
By recording the amount of silver nitrate (AgNO3) is used, the amount of the chloride used is figured. An indicator is used to help determine when the reaction is complete. The indicator used in this experiment is potassium chromate (K2CrO4). The recorded volume of silver nitrate (AgNO3) used is then used to determine the molarity of the silver chloride (AgCl) created. Moles of AgCl = (Volume of AgNO3 added) × (Molarity of AgNO3) Using the molarity of the silver chloride (AgCl) and the atomic weight of the chloride (35.4527), the weight of the chloride from the original unknown chloride salt sample.