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Problem- Calculate the change in pH when 4.00mL of 0.100 M HCl(aq) is added to 100.0mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq).
Calculate the change in pH when 4.00 mL of 0.100 M NaOH(aq) is added to the original buffer solution.
I need expert help to solve the above question. Show each and every step.
Enter scientific notation as 1.23E4. (a) When 11.50 mL of 0.470 M HNO3 have been added. (b) When 65.00 mL of 0.470 M HNO3 have been added
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Write net Bronsted equations and determine the equilibrium constants for the acid-base reactions that occur when aqueous solutions of the following are mixed.
The average water loss during a triathlon is 1.40 L in one hour. The average time to finish a triathlon is 12.6 hours. How much sweat is lost in m^3?
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you have a stock solution of 14.8 m nh3. how many milliliters of this solution should you dilute to make 1000.0 ml of
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