3.) In the assay of NaHCO3, 3.0g of the solid is dissolved in 25mL water. What is the normality? How many mL of 1N H2SO4 will be required to neutralize this solution? From this volume of acid, compute the percent purity of NaHCO3.

1. the temperature for each solution is carried out at approximately 297 K where Kw = 1.00 x 10 ^-14 (a) 0.20 g of hydrogen chloride (HCl) is dissolved in water to make 4.5 L of solution. What is the pH of the resulting hydrochloric acid solution? (b) 0.70 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 3.0 L of solution. What is the pH of this solution ?

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if 5.6g of AI is dissolved in 67000 mls of water, calculate the ppt of Al.

Calculate the percentage CH3COOH in a sample of vinegar from the following data.Sample = 15.00 g,    NaOH used = 43.00 ml ;   0.600 N H2SO4 used for back titration =0.250 ml  ; 1.00ml NaOH is equivalent  to 0.0315 g H2C2O4. 2H2O.

Consider a buffer solution that consists of two separate components: the weak acid, CH3COOH(aq), and its conjugate base, CH3COO¯ (aq)  (added as NaCH3COO).   Which component will react with H+(aq) from a strong acid? Write the net ionic equation for the reaction that occurs when H+(aq) is added to the buffered solution.   Which component will react with OH-(aq) from a strong base? Write the net ionic                  equation for the reaction that occurs when OH-(aq) is added to the buffered solution.

Red cabbage juice is a sensitive acid-base indicator; its colors range from red at acidic pH to yellow in alkaline solutions. If red cabbage is used for the following titration, calculate the pH of the solution described and indicate whether the solution will be red or yellow.    If 67.00 mL of a 1.980 M HNO2 solution is reacted with 2.350 g NaOH, calculate the resulting pH.    Resulting pH = Color of Solution =

Sodium lactate is the sodium salt of lactic acid.a) Use Acid-Base Properties of Salt Solutions, to explain if sodium lactate, NaC3H5O3(aq), is acidic or basic?b) Use ICE table to determine what is the pH of a solution that contains 0.75mol/L lactic acid, HC3H5O3(aq) (Ka = 1.4 x 10-4), and 0.25mol/L sodium lactate, NaC3H5O3(aq) ?

43.  A buffer is prepared using acetic acid, CH3COOH, (a weak acid, pKa = 4.75) and sodium acetate, CH3COONa (which provides acetate ions, the conjugate base), according to the following proportions:   Volume of CH3COOH(aq):   125.0 mL Concentration of CH3COOH(aq):  1.263 M   Volume of CH3COONa(aq):  106.0 mL Concentration of CH3COONa(aq):  1.279 M   Determine the volume of 6.00 M HCl required to change the pH of this buffer by one pH unit.       18.15 mL     36.30 mL     21.87 mL     19.30 mL     43.73 mL

To best accurately determine the molarity of a base, a scientist would need the following: An Erlenmeyer flask, a weighed solid primary standard acid, and NaOH A buret, a weighed solid monobasic base, and an indicator A buret, a weighed solid primary standard acid, and an indicator A buret, a weighed solid primary standard acid, and NaOH A graduated cylinder, a weighed solid primary standard acid, and an indicator