After 25.5 mL of 0.05 M NaOH has been added to 50mL of 0.1 M HF, what is the pH of the solution? (Ka (HF)=7.2*10-4)

Q: Which solution will have the highest pH? The Ka of HClO is 3.8x 10-8 M   A solution of 100 mL of…

A: "Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: For 280.0 mL of a buffer solution that is 0.240 M in HCHO2 and 0.315 M in KCHO2KCHO2, calculate the…

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Q: Calculate the pH of the resulting solution if 0.250 mole of NaOH is added to 500 mL of a buffer…

A: The volume of 1L is equal to 1000 mL. The number of moles (n) of HF is calculated as shown below…

Q: b) A buffer solution is prepared by adding 40.0 g of sodium acetate CH;COONA to 500 mL of a 0.200 M…

A: Given: Mass of CH3COONa =40.0g Molar mass of CH3COONa =82.03 g/mol Volume of solution =500ml=0.5 L…

Q: 20. mL of 0.25 M of HC2H3O2 is titrated with 0.40 M KOH, Calculate the pH of the solution after 15…

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Q: If a buffer solution is 0.200 M in a weak base (Kp = 6.4 x 10-) and 0.480 M in its conjugate acid,…

A: Again.     pH= 14 - pOH Using these two formula pH of the solution can be calculated.

Q: You mix 15.0 mL of 0.200 M NH4Cl with 15.0 mL of 0.400 M NH3. What is the pH of the resulting…

A: Given: Concentration of NH4Cl = 0.200 M Volume of NH4Cl solution = 15.0 mL = 0.015 L…

Q: Calculate the pH resectively after 0.005 moles of NAOH and 0.03 moles of HCl is added into 500 ml of…

A: According to the unit conversion, 500 mL is equal to 0.500 L and molarity of the solution is also…

Q: A buffer solution is 0.486 M in HF and 0.299 M in KF. If Ka for HF is 7.2×10-4, what is the pH of…

A: Given :-  concentration of HF solution = 0.486 M  concentration of KF = 0.299 M  Ka for HF =…

Q: When 0.15 mol of NaOH is added to 2.00 L of 0.600 M HF/ 0.400 M NaF buffer solution, the pH of the…

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Q: buffer was prepared by mixing exactly 200 mL of a 0.60 M NH3 solution and 300 mL of a 0.30 M NH4Cl…

A: Given that: volume of NH3 = 200 mL = 0.2 L, molarity = 0.60 M Volume of NH4Cl = 300 mL = 0.3 L and…

Q: If a buffer solution is 0.280 M in a weak base (K, = 5.7 x 10-5) and 0.450 M in its conjugate acid,…

A: We have to predict the pH of the solution.

Q: 1. 50.0 ml of 0.1 M NaOH is added to 100.0 ml of 0.2 M HCN (Ka=6.2x10-10). What is the pH of the…

A: Since you have posted multiple questions, we are entitled to answer the first only. 1) Given:…

Q: 5.0 mL of 0.100 M NAOH is added to 50.0 mL of 0.100 M hypochlorous acid (HCIO). If the K, of…

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Q: What is the pH of a 80.0 mL solution of 1.25 M concentration acid HA after 40.0 mL of 2.00 M…

A: Equation for the reaction of the monoprotic acid, HA and NaOH is: HA(aq) + NaOH(aq)   ---->…

Q: What is the pH of the buffered created by dissolving 60.0g HCN (MM= 27.0253 g/mol) and 60.0g KCN…

A: The PH can be calculated as follows

Q: 20.00 mL of 0.100 M sodium hydroxide is added to 40.00 mL of a 0.100 M acetic acid solution. The Ka…

A: Given data: Volume of sodium hydroxide = 20.00 mL = 0.02 L, Concentration of sodium hydroxide =…

Q: 8) Given a buffer solution that is 0.250 M in formic acid (HCOOH) and 0.150 M sodium formate…

A: From given data  Formic acid concentration [Acid]= 0.250 M Sodium formate concentration [Salt]=…

Q: )What is the pH of the buffer solution?   b)What would the pH above the buffer in #3 be after…

A: The question is based on the concept of buffer solution.   A buffer is a solution which resist any…

Q: 50.0 ml of 0.1 M NaOH is added to 100.0 ml of 0.2 M HCN (Ka=6.2x10-10). What is the pH of the…

A: A buffer solution is a mixture of weak acid and its conjugate base or weak base and it's conjugate…

Q: You add 19.00 mL of 0.800 M NaOH to 50.00 mL of pure water, and to this mixture you then add 7.00 mL…

A:

Q: When 25.0 mL of 0.400 M hydrobromic acid and 25.0 mL of 0.400 M potassium nitrite are combined, the…

A: Given that: the volume of hydrobromic acid= 25.0 mL = 0.025 L molarity of hydrobromic acid= 0.400 M…

Q: A buffer solution is 0.374 M in H2 S and 0.205 M in KHS. If Ka1 for H2S is 1.0 x 10-7, what is the…

A: when a weak base and its salt are present in solution, they form a buffer solution.

Q: [4} What is the pH of the solution in the flask after 25.00 mL of 0.110 M NAOH has been added to…

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Q: For 240.0 mL of a buffer solution that is 0.195 MM in HCHO2 and 0.295 M in KCHO2, calculate the…

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Q: How many moles of NH4Cl must be added to 2.0 L of 0.10 M NH3 to form a buffer whose pH is 9.00?…

A: Given : Volume of solution = 2.0 L Concentration of NH3 = 0.10 M And pH of the buffer solution =…

Q: Suppose you have just added 100.0 ml of a solution containing 0.5000 moles of acetic acid per liter…

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Q: calculate the PH after 15.0 ml of 0.10M NaOH has been added to 100.0 ml of a butter that is 0.50 M…

A: Given-> Volume of NaOH = 15.0 ml  Molarity of NaOH = 0.10 M Volume of buffer = 100.0 ml Molarity…

Q: A buffer is prepared by adding 45 ml of 0.15 NaF to 35 ml of 0.1 M HF. What is the pH of the final…

A: Interpretation -  To determine the pH of the final solution when a buffer is prepared by adding 45…

Q: How much 5.50M  NaOH must be added to 550.0 mL of a buffer that is 0.0190 M  acetic acid and 0.0245…

A: The question is based on the concept of buffer solution.   A buffer is a solution which resist any…

Q: A buffer solution is 0.384 M in H2S and 0.210 M in KHS. If Kal for H2S is 1.0 × 10-7, what is the pH…

A:

Q: Consider a 1.0-L solution that is initially 0.500 M NH3 and 0.570 M NH4CI at 25 °C. What is the pH…

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Q: 4. What is the pH of a buffer solution consisting of 0.0550 M NH3 and 0.0800 M NH. (K, for NH is 5.6…

A: Given-> [NH3] = 0.0550 M [NH4^+] = 0.0800 M Ka(NH4^+] = 5.6 × 10^ -10

Q: 1. A student has available 1L of a buffer solution: 0.55M acetic acid and 0.45 M sodium acetate.…

A: GIVEN:

Q: What is the pH after 50.0 mL of 0.200 M NaOH has been added to 300.0 mL of a buffer solution…

A: Given: Concentration of HX = 0.74 M Concentration of X- = 0.43 M Concentration of NaOH = 0.200 M…

Q: A buffer is prepared by adding 45.0 mL of 0.15 M NaF to 35.0 mL of 0.10 M HF. What is the pH of the…

A: A buffer is a solution that may be a mixture of a weak acid and its salt or a weak base and its salt…

Q: Moly Cule is titrating 0.2 M of a strong base (NaOH) into 100 ml of a solution of 0.1M weak acid…

A: Given: Molarity of NaOH  = 0.2 M Volume of solution = 100 mL Molarity of HAc     = 0.1 M Ka for HAc…

Q: 25.00mL of a 0.100 M sodium hydroxide is added to 45.00 mL of a 0.100 M acetic acid solution. The Ka…

A: Reaction CH3COOH + NaOH ------------> CH3COONa  +  H2O  Volume of acetic acid = 45 mL Molality of…

Q: Calculate [OH] in a solution obtained by adding 1.90 g solid KOH to 1.00 L of 10.0 M NH3. (Kb of NH3…

A: KOH is a strong base, whereas NH3 is a weak base.

Q: How much 5.50 M NaOH must be added to 580.0 mL of a buffer that is 0.0200 M acetic acid and 0.0275 M…

A:

Q: Calculate the pH of a buffer solution that is 0.200 M in HCN and 0.120 M in NaCN.  The Ka of HCN is…

A: Given that : The concentration of acid (HCN) = 0.200 M The concentration of salt (NaCN) = 0.120 M…

Q: What is the pH of the solution that results from adding 24.7 mL of 0.11 M HCl to 25.2 mL of 0.41 M…

A:

Q: What is the pH of a buffer made by dissolving 0.2 mol of KBrO and 0.6 mol of HBrO in 850 mL of…

A: Interpretation -  To determine the pH of of a buffer made by dissolving 0.2 mole of KBrO and 0.6…

Q: At 22 °C, an excess amount of a generic metal hydroxide, M(OH),2, is mixed with pure water. The…

A:

Q: When a strong base is added to buffer it will react to become neutralized. Determine the pH after…

A: From the Henderson-Hasselbalch equation: Since, Ka = 5.8×10-10 Therefore,

Q: A buffer solution is made up of 1.0 M NH3 and 1.0 M NH4CI. = 1.8 x 10-5 K₂NH3 What is the pH when 20…

A: Given :  Volume of buffer solution= 25. ml  Concentration of NH3 = 1.0 M  Concentration of NH4Cl =…

Q: A beaker contains 100. mL of the buffer solution. What is the resulting pH when 50.0 mL of 0.4 M…

A: Given the total volume of the buffer solution, V = 100 mL  Molarity of H2PO4-(aq) in the buffer…

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.