If a solution containing 123.67 g of silver nitrate is allowed to react completely with a solution containing 11.85 g of lithium hydroxide, how many grams of solid precipitate will be formed?   How many grams of the reactant in excess will remain after the reaction?   Assuming complete precipitation, how many moles of each ion remain in solution? If an ion is no longer in solution, enter a zero (0) for the number of moles.   Li+:   OH-:   Ag+:   NO3-:

Use the Conservation of Mass Interactive to answer the question. Consider the reaction. MnS (s) + 2HCl(aq) →→→MnCl₂ (aq) + H₂S(g) If the large amount of MnS is combined with the large amount of HCI, what is the mass of the products? The mass of any excess reactants will also be included in this total. mass: A 12.49 g sample of NaBr contains 22.34% Na by mass. Considering the law of constant composition (definite proportions), how many grams of sodium does a 8.61 g sample of sodium bromide contain? g & Na average atomic mass= On another planet, the isotopes of titanium have the given natural abundances. Isotope Abundance Mass (u) 46Ti 74.900% 45.95263 4871 18.800% 47.94795 50Ti 6.300% 49.94479 What is the average atomic mass of titanium on that planet? U

Which of the following pairs of solutions will give a precipitate when mixed?    Sodium phosphate and calcium perchlorate. Mercury (II) nitrate and sodium chloride.    Ammonium chloride and calcium acetate.  Silver nitrate and sodium acetate.   Sodium sulfate and copper (II) chloride.

Complete the table below by deciding whether a precipitate forms when aqueous solutions A and B are mixed. If a precipitate will form, enter its empirical formula in the last column. solution A solution B Does a precipitate form when A and B are mixed? empirical formula of precipitate ? iron(II) bromide sodium hydroxide yes O no copper(II) chloride ammonium sulfide yes no zinc nitrate manganese(II) chloride yes no