Question

Sodium hydroxide solutions are common in chemical manufacturing, used in everything from the production of soaps to explosives.

a. How could a chemist prepare 5.0 L of a 2.0 M aqueous stock solution of sodium hydroxide?

b. Through dilution of the stock solution in Part a, how could a chemist prepare 250 mL of 0.5 M aqueous sodium hydroxide solution.

c. To safely dispose of solutions of strong bases like sodium hydroxide, it is necessary to first neutralize them by reaction with an acidic solution. Write and balance the molecular equation for the reaction of aqueous sodium hydroxide with aqueous sulfuric acid. .

d. What volume of a 0.5 M solution of sulfuric acid would be necessary to neutralize the 250 mL 0.5 M sodium hydroxide solution prepared in Part b.

Answer 1

Number of melas otNao 2 0 mot 5-0 L Io. mu) mass of Neo Males M0 glmu Mass af NauHlo. melxe = ५०० DiSsalve 4o0 Sol Naa in amunnt minmam Sand dlute Solntoh to S.o lL M VI O.S M 2S0 ml 2 0 O5250 62-5 ml 2 DIhe 62-S mL o 2-0 Shoe Snh to 2S0 mL

Mo S + H० ५ D«0 \ + AS० > 2 ২ १ bo\~n\९ Mos b 2 ० Me0H. 2NaoHt HSD Benlnnie ०९ ०০০ Cogosaunt M~ S০ + H O ২ ০১- ২ 2 20e0\A + h s 0 ।N, S ० +2 नैसर N ২ ৯ -0Smol ) ২S 0+ M«DH ८S० m ०\९९ m० ) 1ov m/L ई ) २ ০. ০ ৫ ८5 ০-\25 wi mu) रा ২ hsaSuaey ০-S ৩ } Valnm "१ ০ ০625 mo) (० ০ ৩ । ा mul ০S L 12S mL