#90cm^3# of 0.01M calcium hydroxide were added to a sample of water containing 0.001 moles of calcium hydrogen carbonate.
(a) Write an equation for the reaction which took place
(b) Calculate the number of moles of calcium ions in #90cm^3# of 0.01M calcium hydroxide.

Answer:

a)
#Ca(OH)_2(aq)+Ca(HCO_3)_2(aq)#
#rightarrow2CaCO_3(s)+2H_2O(l)#

b)moles=#(volume timesMolarity)/(1000)#,

Moles of #Ca^(2+)=(90times0.01)/1000#

=0.0009 moles

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#90cm^3# of 0.01M calcium hydroxide were added to a sample of water containing 0.001 moles of calcium hydrogen carbonate. (a) Write an equation for the reaction which took place (b) Calculate the number of moles of calcium ions in #90cm^3# of 0.01M calcium hydroxide.

#90cm^3# of 0.01M calcium hydroxide were added to a sample of water containing 0.001 moles of calcium hydrogen carbonate.
(a) Write an equation for the reaction which took place
(b) Calculate the number of moles of calcium ions in #90cm^3# of 0.01M calcium hydroxide.