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- Ammonia gas is bubbled into 275 mL of water to make an aqueous solution of ammonia. To prepare a buffer with a pH of 9.56, 15.0 g of NH4Cl are added. How many liters of NH3; at 25C and 0.981 atm should be used to prepare the buffer? Assume no volume changes and ignore the vapor pressure of water.Determine the pH of a 0.650 M solution of magnesium nitrite, Mg(NO2)2 at 25 °C. A solution containing 7.50 g of this salt is diluted with water until it reaches a pH of 8.18.What is its final volume? Give one example of a salt whose solution is expected to be acidic and briefly explain why. Give one example of a salt whose solution is expected to be basic and briefly explain why. You cannot reuse the compound in a) and b) to answer c) and d).How many milliliters of 0.800 M KOH should be added to 3.38 g of oxalic acid (C2O4H2) to give a pH of 4.40 when diluted to 500 mL? [For oxalic acid pK, = 1.250 and pK2 = 4.266]
- 1. Calculate the pH of a 0.594 M aqueous solution of pyridinium chloride, C5H5NHCl. The Kb of pyridine is 1.8 x 10-9. The answer must be given with the correct number of significant figures. 2. How many grams of NaF must be added to 60.0 mL of 0.500 M HF(aq) to adjust the pH to 3.40? Assume no volume change. The pKa of HF is 3.14.A) At 25°C, a 0.21 M solution of diethylamine, (C2H6)2NH that acts as a weak base, is 4.0% ionized. What is Kb for diethylamine? Kb = __________ B) What is the pH of a solution obtained by mixing 0.75 L of 0.185 M Ba(OH)2 and 0.14 L of 0.106 M HCl? Assume that volumes are additive. pH = _________HCl and Na2CO3 undergo a neutralization reaction. To neutralize the acid and base, 0.0144L of 3.2913M HCl is required, and 0.0251 of 0.9435M Na2CO3 is required. To make sure the volumes of HCl and Na2CO3 neutralize the reaction properly, calculate the pH of the solution to see if the solution is fully neutralized (pH of 7 or close to 7).
- what is the pH of a solution prepared by adding 63.6 mL of 0.100 M sodium hydroxide to 69.37 mL of 0.829 M benzoic acid (Ka=6.14x10^-5)?the answer I got for this question is wrong, along with quite a few I have asked in the past. The Ph of a weak acid and strong base is not 7. It does not work that way. Þú byrjar með 100.0 mL af 0.250 M HCN og bætir við 0.750 M NaOH við 25°C. (HCN Ka = 6.2 * 10-10.) You begin with 100 mL of 0,250 M HCN and add to it 0,75 M NaOH at 25°C (HCN Ka = 6,2 * 10-10) Calculate the pH at the equivalence point. / Calculate the pH after 150 mL of NaOH has been added. Can you please check this answer and help me out https://www.bartleby.com/questions-and-answers/you-begin-with-100-ml-of-0250-m-hcn-and-add-to-it-075-m-naoh-at-25c-hcn-ka-62-10-10-calculate-the-ph/9cc945c7-a648-46e2-8057-4c800a5eb855The pH of dissolving 1.48g of propanoic acid in 200ml of H2O is ---- If Ka=1.3*10^-5
- You add 100.0 mL of 0.50 M NaOH to 50.0 mL of 1.00 M NH4CI. What is the pH of the resulting solution? Kb (NH3)=1.8x10-5 11.602.6111.399.34What is the pH of a solution prepared by combining 0.258 mol of a newly discovered weak acid (Ka = 1.3 x 10-4) with 0.156 mol of the salt containing its conjugate base in 1.4 L of water?Twenty millimeters of 0.50N HOAc is diluted with water to 100mL, and the resulting solution is titrated with 0.50N HOAc. Calculate the pH value (a) at the start, (b) when 0.8 ml of the NaOH has been added, (c) at the equivalence point (when 20mL of NaOH has been added, (d) when 30mL of the NaOH has been added. Ka=1.8x10^-5