2 Al (s) + 2 KOH (aq) + 6 HOH (l) ---> 2 KAl(OH)4 (aq) + 3 H2 (g) Under experimental procedures #2 and #3, the experiment calls for reacting aluminum with water and potassium hydroxide. See above for the equation. A student using quantities: 3.00 grams Al 15.0 mL of 8.00 M KOH 75.0 mL distilled HOH Which of the reactants is the limiting reactant? (Mathematically document this.) Show your work and set up.

In a titration experiment, a 5.00-mL sample of sulfuric acid, H2SO4, from a car battery is diluted with de-ionized water to 100.0 mL. A 20.00-mL portion of the diluted acid is titrated with 0.2025 MNaOH solution. If 42.00 mL of the NaOH solution is required to neutralize the dilute acid, what is the molar concentration of H2SO4 in the original solution taken from the battery? The acid-base reaction occurs as follows:                 H2SO(aq)  +  2NaOH(aq)   -->  Na2SO4(aq)  +  2H2O(l)          (A) 0.2126 M                             (B) 0.4252 M                             (C) 4.25 M                     (D) 8.50 M

Please write the molecular equation when mixing the following two aqueous salts: P b ( N O 3 ) 2 ( a q ) + K I ( a q ) ⟶ ???     ***All chemical equations must be balanced, have proper subscripts/superscripts, and list the state of the chemical***

Predict the reactants of this chemical reaction. That is, fill in the left side of the chemical equation. Be sure the equation you submit is balanced. (You can edit both sides of the equation to balance it, if you need to.) Note: you are writing the molecular, and not the net ionic equation. 0 - H,0(1) NaF (aq) +

Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory to standardize strong base solutions. It has the unwieldy formula of KHC8H4O4. This is often written in shorthand notation as KHP.What volume of a 0.370 M barium hydroxide solution is needed to exactly neutralize 4.24 grams of KHP ?

Consider the following reaction H2S (g) + FeS(s) + CO2(g) →FeS2(s) + HCO2H(aq) If 2.00 g of each reactant is each dissolved in 250.0 mL of water and all the solutions are mixed together. The final volume was measured to be 750.0 mL.  a)How many grams of CO2 left unreacted?  b) What is the concentration of HCO2H in this solution?

Predict the reactants of this chemical reaction. That is, fill in the left side of the chemical equation. Be sure the equation you submit is balanced. (You can edit both sides of the equation to balance it, if you need to.) Note: you are writing the molecular, and not the net ionic equation. [] --> Ba(ClO3)2 (aq) + H2O (l)

How many grams of PbBr2 will precipitate when excess NaBr solution is added to 72.0 ml of 0.791 M Pb(NO3)2 solution? Pb(NO3)2(aq) + 2NaBr(aq) PbBr2(s) + 2NANO3(aq)

1) A 1.20 gram sample of ammonium phosphate is dissolved in 100. mL of water. The solution is poured into 50.0 mL of a 1.5 M magnesium nitrate solution. What mass (g) of solid product will be produced if the reaction runs to completion? Concentration of  M of NH+4NH4+ (M)? Concentration of  M of PO3−4PO43− (M) Concentration of  M of Mg2+Mg2+ (M) Concentration of  M of NO−3NO3− (M)

A 2.00 g sample of KCl is dissolved in 60.0 mL of water. The resulting solution is then added to 20.0 mL of a 0.830 M CaCl2 (aq) solution. Assuming that the volumes are additive, calculate the concentrations of each ion present in the final solution. Concentration of K+ ions = M Concentration of Ca 2+ ions = M Concentration of Cl¯ ions = M