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1.What is the percent relative uncertainty of pH of a 0.1861(±0.0004) molar solution of HCl?
pH=−logMHcl
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- Q3. This question is about the pH of several solutions. Give all values of pH to 2 decimal places. (a) (i) Write an expression for pH. (b) (ii) Calculate the pH of the solution formed when 10.0 cm³ of 0.154 mol dm-³ hydrochloric acid are added to 990 cm³ of water. The acid dissociation constant, Ka, for the weak acid HX has the value 4.83 x 10-5 mol dm-³ at 25 °C. A solution of HX has a pH of 2.48 Calculate the concentration of HX in the solution. Page 4 of 146. (i) Define pH in words. The strong acid HClahas a pH value of 1, use the following equation for a strong acid: H+, + and convert the following expression to deduce the hydrogen ion concentration: pH = -log10 [H*] (ii) Use the above expression to deduce the pH of HCL (ag) given the concentration of the acid to be 4.5 mol/dm3 pH =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.
- in 2.1M CH3NH2 aqueous solution, determine the percentage of ionised CH3NH2 molecules. Kb = 4.4*10^-424. A solution of volume 0.500 L contains 1.68 g NH3 and 4.05 g (NH4)2SO4. (a) What is the pH of this solution? (b) If 0.88 g NaOH is added to the solution, what will be the pH? (c) How many milliliters of 12 M HCl must be added to 0.500 L of the original solution to change its pH to 9.00?The ionization constant of lactic acid, CH,CH(OH)CO,H, an acid found in the blood after strenuous exercise, is 1.36 x 10-4. What is the concentration of hydronium ion in the solution of 0.102 M lactic acid? CH;CH(OH)CO,H (aq) + H,O (1) → H;O• (aq) + CH;CH(OH)CO, (aq) O 0.00372 M O 0.0165 M O 0.00549 M O 0.227 M
- 6. (i) Define pH in words. The strong acid HClag has a pH value of 1, use the following equation for a strong acid: HClaa Hog + and convert the following expression to deduce the hydrogen ion concentration: pH = -log10 [H+] Clea (ii) Use the above expression to deduce the pH of HCl (ag) given the concentration of the acid to be 4.5 mol/dm³ pH =(i) Define pH in words. The strong acid HClaq has a pH value of 1, use the following equation for a strong acid: HClaq à H+aq + Cl-aq and convert the following expression to deduce the hydrogen ion concentration: pH = -log10 [H+] (ii) Use the above expression to deduce the pH of HCl (aq) given the concentration of the acid to be 4.5 mol/dm3 pH =(i) Define pH in words. The strong acid HClaq has a pH value of 1, use the following equation for a strong acid: HClaq à H+aq + Cl-aq and convert the following expression to deduce the hydrogen ion concentration: pH = -log10 [H+] (ii) Use the above expression to deduce the pH of HCl (aq) given the concentration of the acid to be 4.5 mol/dm3
- What is the pH of a 0.0556 M NH, (aq) solution at room temperature? The base ionization constant of ammonia is K, = 1.8×10. Enter your answer in the box provided with correct %3D units and sig. figs.: The pH of 0.0556 M ammonia is : pH %3DCalculate the molar concentration of OH− ions in a 0.077 M solution of ethylamine (C2H5NH2; Kb=6.4x10-4If 44.97 ml of a solution of HCl are equivalent to 43.76 ml solution of NaOH, and if 49.14 ml of the latter will neutralize 0.2162 g of KHC2O4.H2C2O4.2H2O, what volume of water should be added to a liter of the HCl in order to make it 0.0500 N?