A tablet containing 500 mg of aspirin was dissolved in enough water to make 100 mL of solution. Given that Ka = 3.0x10^-4 for aspirin, what is the pH of the solution?

Calculate the pH of a 0.054M HA(aq) solution where HA is a strong acid. pH = キキ, *assume the temperature is 25°C.

Suppose that 42.00 mL of 0.150 M NaOH is added to 0.360 g of a weak acid, H3A.  The excess NaOH is then titrated with 23.40 mL of 0.120 M HCl.   What is the molar mass of the acid? a) 103 g/mol b) 241 g/mol c) 190 g/mol d) 310 g/mol

||| ctrl lacc shift ↑ tab caps lock VILION Mc ALE Graw HI esc K →1 Pavilion x360 fn O CHEMICAL REACTIONS Determining the molar mass of an acid by titration McCA X Eplanation g mol V An analytical chemist weighs out 0.188 g of an unknown triprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1500M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 38.4 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. f1 Type here to search A https://www-awu.aleks.com/alekscgi/x/Isl.exe/1o_u-IgNslkr7j8P3jH-IvUrTNdLZh5A8CnG03PBGuXr8iCPa7ZMmym f2 @ Z Check 2 L M W hp S ALE MCCA ALER f3 # Mc Graw 3 X alt D 4 $ 4 с x10 X R O f5 Me Graw MI % F 5 at 40 MCCA ALE ALE ● V T S f6 4- G 6 ■ T f7 B Y ♫+ & Mc 7 H raw fg MCCA ALER *. N KAA © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center |…