This is a Numeric Entry question/ It is worth 3 points/You have 10 of 10 attempt

Question

This is a Numeric Entry question/ It is worth 3 points/You have 10 of 10 attempts /There is no attempt penalty a See page 170 4 Question (3 points) 1st attempt See Periodic Table ’See Hint An aqueous solution containing both Srt and CO,2 ions is mixed in order to precipitate SrCO(s). Given there are 1.25 mL of 267 M Sr2+ ions, calculate the mass of SC03 that is formed. Assume that all of the Sr2+ ions are consumed. The net ionic reaction is shown below. Sr2 + (aq)+CO!"(aq) SrCO3(s) 343s 31 OF 38

Explanation / Answer

Moles of Sr^2+ ions = 1.25 mL * (2.67 mol/1000 mL) => 0.0033375 moles

1 equivalent of Sr^2+ ions will form 1 equivalent of SrCO3 molecules

So 0.0033375 moles of Sr^2+ ions will form 0.0033375 moles of SrCO3

Molar mass of SrCO3 = 147.62 g/mol

So 0.0033375 mol * 147.62 g/mol

= 0.49 g of SrCO3

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