Solution Stoichiometry and Net Ionic Equations

How many moles of BaCl₂ are formed in the neutralization of 393 mL of 0.171 M Ba(OH)₂ with aqueous HCl?

• 1.15 mol

• 0.0672 mol

• 0.0336 mol

• 2.30 mol

Tags

NGSS.HS-PS1-7

What mass of the solid precipitate is formed when 35.5 mL of 0.184 M AgNO₃ is treated with an excess of aqueous hydrobromic acid?

• 53.6 g

• 1.44 g

• 1.23 g

• 34.5 g

Aqueous solutions of sodium chloride and lead (II) nitrate react to form solid lead(II) chloride. What is the mass of the solid product if 250.0 mL of 1.75 M sodium chloride reacts with excess lead(II) nitrate?

• 78.5 g

• 93.1 g

• 45.5 g

• 60.8 g

• 59.4 g

18.26 mL of a 1.50M hydrochloric acid reacts with magnesium hydroxide. Calculate the mass of magnesium hydroxide needed for the reaction. 
  Mg(OH)₂  +  2 HCl  ->  2 H₂O + MgCl₂           

• 4.68 g Mg(OH)₂
• 0.789 g Mg(OH)₂
• 0.0274 Mg(OH)₂
• 1.07 g Mg(OH)₂

Tags

NGSS.HS-PS1-7

What precipitate forms when you mix lead (II) nitrate with sodium chloride?

• sodium nitrate 
• lead (II) chloride 
• sodium lead
• chloride nitrate 

Which is the correct net ionic equation for the reaction of AgNO₃ and CaCl₂?

• Ca²⁺(aq) +  2Cl^- (aq) → CaCl(s)
• Ag⁺(aq)  +  Cl^- (aq) → AgCl(s)
• Ag +  Cl  →  AgCl
• Ag⁺  +  Ca²⁺   →Ag₂Ca (s)

Which of these results in formation of a precipitate?

• BaNO₃(aq)  +  NaCl(aq)→
• KNO₃(aq)  +  LiOH(aq)→
• Zn(NO₃)₂(aq)  +  NaOH(aq)→
• NaNO₃(aq)  +  Ba(OH)₂(aq)→

What are the spectator ions in this reaction?
CuCl₂(aq) + NaOH(aq) → Cu(OH)₂(s) + NaCl(aq)
 

• Cu²⁺ and OH^1-
• Na²⁺ and Cl^2-
• Na¹⁺ and Cl^1-
• Na¹⁺ and OH^1-