For each of the following unbalanced equations,
calculate how many moles of the second reactant
would be required to react completely with
exactly 25.0 g of the first reactant. Indicate
clearly the mole ratio used for each conversion.
a. Mg(s) + CuCl2(aq) → MgCl2(aq) + Cu(s)
b. AgNO3(aq) + NiCl2(aq) →
AgCl(s) + Ni(NO3)2(aq)
C. NaHSO3(aq) + NaOH(aq) →
Na2SO3(aq) + H2O(l)
d. KHCO3(aq) + HCl(aq) →
KCl(aq) + H2O(l) + CO (g)

Idon't have a clue what this

Answer:     c. lso₄======since cl has an ion charge of -1, the formula    tells us that l has an ion charge of +2 because we needed two chloride ions to fully empty out the valence shell of l, hence the 1: 2 ratio of l to cl.  each chloride ion needs only 1 electron to fully fill their valence shells.since so₄ has an ion charge of -2, it will accept two electrons to get a full valence shell. we established that l has an ion charge of +2. these charge numbers are the same; l will provide the two electrons needed. it's a 1: 1 ratio between l and so₄the formula would therefore be lso₄

Awould be the answer you would want

75 degres hope thois