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What is the pH of a solution of 40.0 mL of 0.100 M acetic acid (Ka = 1.8 x 10-5) after 50.0 mL of 0.100 M NaOH has been addedCalculate the concentration of dissolved Ba2+ ions when BaSO4 is added to water at 25°C. Кsp? = 1.10 x 10-10A particular saturated solution of silver chromate (Ag2CrO4), has [Ag+] = 5.0 x 10 Mand (CrO4) = 4.4 x 10M. What is value KspAs a result of mineral erosion and biological activity, phosphate ion is common in natural waters. If [Ca 2+] = 1 x 10-6 M anWhat is the pH at the equivalence point in the titration of 100.0 mL of 0.0500 M HOCI (Ka = 3.5 x 10-8) with 0.400 M NaOH? ExA certain weak acid, HA, with a Ka value of 5.61 x 10-6, is titrated with NaOH. Part A A solution is made by titrating 8.00 m

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Solufior biven, V = 40mL Cool M Acetic Acid Ka = 1.8 x105 V2 = 50mL Ca D.IM Noor H2014) - hero V Balanced chemical equation CKg = log (1.8 x1005 pka tog pka = 4.74 4.74 + PH 4.74 + dog (0:014 0.0 444 pH = 4.138 Aug

Bro, which question answer do you want...it's not clear very confusing...

I have solved the first one...

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