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+//To Find the Concentrations of all the species in the reaction
+
+//Example 11.3
+
+clc;
+
+clear;
+
+Ka=4.2*10^-7;//Acid Dissociation Constant for Carbonic Acid
+
+Sol=1.1*10^-5;//Solubility of CO2 in equilibrium with water
+
+a1=1;b1=Ka;c1=-Ka*Sol;//Coefficients a,b and c of the quadratic equation to find the concentration of H+
+
+d1=(b1^2-(4*a1*c1));//Discriminant of the Quadratic Equation
+
+x=(-b1+sqrt(d1))/(2*a1);//Concentration of H+
+
+Ka2=4.8*10^-11;//Second Dissociation Constant for H2CO3
+
+y=Ka2;//Concentration of CO3 2- ions
+
+Kw=1*10^-14;//Disscociation Constant of Water
+
+z=Kw/x;//Concentration of OH- ions (The answer vary due to round off error)
+
+printf("At Equilibrium the concentrations are as follows:");
+
+printf("\n [H+]=%.1f*10^-6 M",x*10^6);
+
+printf("\n [OH-]=%.1f*10^-9 M",z*10^9);
+
+printf("\n [H2CO3]=%.1f*10^-5 M",Sol*10^5);
+
+printf("\n [HCO3-]=%.1f*10^-6 M",x*10^6);
+
+printf("\n [CO3 2-]=%.1f*10^-11 M",y*10^11);