Explanation :
NH4NO3 is formed from strong acid and weak base. so this is added to NH3 , then it is acidic. so pH decreases.
Na2CO3 is formed from strong base and weak acid. so this is basic. pH increases.
NaClO4 is neutral . so no change in NaOH pH.
Question 3 (1 point) Determine whether the pH will increase, decrease, or remain the same when th...
Predict whether the solubility of CoCO3(s) will increase, decrease, or remain the same upon addition of each of the following substances (Co2 can form complex ions (Co(CN).] when in presence of CN lons) (a) Hl(aq) (b) Co(NO3)2(aq) (c) Na2CO3(aq) (d) LICN(aq)
Does the pH of the solution increase, decrease, or stay the same when you add solid sodium hydrogen oxalate, NaHC2O4 to a dilute aqueous solution of oxalic acid, H2C2O4? Explain your answer using the equation below. H2C2O4 (aq) + H2O (l)⇌ HC2O41– (aq) + H3O+ (aq) 2)Why a solution of sodium chloride and hydrochloric acid cannot act as a buffer? (b) Propose a conjugate acid/base pair which can function as a buffer. 3) (a) Calculate the pH of a buffer...
Question 3 (1 point) A buffer solution is made by adding 15.0 mL of a 0.50 M Na2CO3 solution to 15.0 mL of a 0.50 M NaHCO3 solution in a test tube. 2.4 mL of a 1.0 M HCl solution is added to this buffer solution. What is the final pH of the solution in the test tube? H2CO3 has Ka1 = 4.3×10-7 and Ka2 = 5.6×10-11. Question 4 (1 point) A buffer solution is made by adding 10.0 mL...
A buffer solution contains 0.386 M NaHCO3 and 0.233 M Na2CO3. Determine the pH change when 0.055 mol HI is added to 1.00 L of the buffer. pH change = Determine the pH change when 0.117 mol NaOH is added to 1.00 L of a buffer solution that is 0.498 M in HCIO and 0.235 M in C10". pH after addition - pH before addition = pH change =
10. Which of the following mixtures has lower pH a) Equal volumes of 0.10M HCIO, and 0.10M NaOH b) Equal volumes of 0.10M HCIO and 0.10M NH Ans: 1. Does the pH increase, decrease or remain same on addition of each of the following a) NH4NO) to NHs solution Ans: b) Na:CO) to NaHCO3 solution Ans: c) NaCIO4 to NaOH solution Ans: 12. Which of the following solutions give a buffer solution when equal volumes are mixed? a) 0.10M NaF...
Question 5B: pH Changes Due to the"common ion effect," when the salt NaC3H,03 is added to an aqueous solution of the weak acid HC H,O3 will the following concentrations increase, decrease, or remain the same? b) HO c) IOH Question 5B: pH Changes Due to the"common ion effect," when the salt NaC3H,03 is added to an aqueous solution of the weak acid HC H,O3 will the following concentrations increase, decrease, or remain the same? b) HO c) IOH
Question 1 (1 point) 12.0 mL of a 0.50 M Na2CO3 solution is added to a large test tube. Enough 0.50 M NaHCO3 solution is added to the test tube to give a final volume of 30.0 mL. What is the pH of the resulting buffer solution? H2CO3 has Ka1 = 4.3×10-7 and Ka2 = 5.6×10-11. Question 3 (1 point) A buffer solution is made by adding 15.0 mL of a 0.50 M Na2CO3 solution to 15.0 mL of a...
Fill in the blanks with increase, decrease, or remain the same to correctly complete each statement. (1) Contribution margin ratio will with an increase in sales volume. (2) Fixed cost per unit will with an increase in sales volume (within the relevant range). (3) A decrease in the contribution margin will cause the break-even point to (4) Variable cost per unit will with a decrease in sales volume. (5) An increase in fixed costs will cause the break-even point to...
Fill in the blanks with increase, decrease, or remain the same to correctly complete each statement: 1. Contribution margin ratio will _________ with an increase in sales volume. 2. Fixed cost per unit will_______ with an increase in sales volume (within the relevant range) 3. A decrease in the contribution margin will cause the break-even point to __________. 4. Variable cost per unit will _________ with a decrease in sales volume. 5. An increase in fixed costs will cause the...
Determine the pH increase of a solution after 0.10 mol of NaOH is added to 1.00 L of a solution containing 0.15 M HC2H3O2 and 0.20 M NaC2H3O2. If this same amount of NaOH was added to 1.00 L of pure water then what would be the pH increase of the resulting solution? Compare these two values. pH increase in buffer: ? pH increase in pure water: ?