Dimensional analysis

If an aluminum sphere has a mass of 23.01 grams and was heated to 137.0 Celsius and lowered into a cup containing 20.00 mL of water at 21.0 Celsius. The final temperature of the water and the sphere was 44.0 Celsius assuming no heat was loss calculate the specific heat of the aluminum in the sphere. C h2o =4.184J/g-0celsius q=m x C x ( t final - T initial) I can not figure where to input the figures to receive a logical answer

Chemical reactions

In a double replacement what comes from or forms from ___Cu(NO3)2 (aq) +__ NaOH (aq) What about __Fe(NO3)3 (aq) + __NaOH (aq)?

This question deals with aluminum chemistry and the formation of aluminum hydroxide from aluminum sulfate and water

Assume we have a 1000L tank of water and very dilute weak acids. To this tank we add and dissolve 260 grams AL2(SO4)3 (solid granules) --- the resultant pH is 4. The intention is to form AL(OH)3 solids/particles in this reaction. Question 1: How much Al(OH)3 will be formed in this reaction at pH=4.0 Question 2: If the pH were raised to 5.5 with NaOH, there is an appearance of more AL(OH)3 being formed ---- why? And, how much more aluminum hydroxide would be formed at this higher pH? Question 3: It also appears that not all of the alum (aluminum sulfate) dissolves in water and therefore limits the max. creation of aluminum hydroxide --- why?

Calculating mass of sulfuric acid to affect pH change?

I have a 2 part question concerning the use of H2SO4 to adjust the pH of a solution: 1. How many grams per liter of H2SO4 is required to adjust the pH of a solution from 3.8 to 2.8 assuming the sulfuric acid fully ionizes? 2. If in reality however, the actual sulfuric acid ionization/dissociation is a 2 step process and not fully ionized such that: If, K1 = [H+][HSO4-]/[H2SO4] is complete and is equal to 100 mol/L, But if the second reaction is not complete such that: K2 = [H+][HSO4--]/[HSO4-] is incomplete and equal to .012 mol/L, then how many grams/liter of sulfuric acid in this case would be required to change the pH of the solution from 3.8 to 2.8?

pH adjustment of a solution with NaOH or Ca(OH)2?

Assume you have a 64000L volume of solution (predominantly water) with a pH of 4.03. 1. How much NaOH would be required to raise the pH to 5.5? 2. Or, if using Ca(OH)2 --- how much calcium hydroxide would be required to raise the pH of this solution to 5.5? In each case, assume full ionization of the base.