Suppose you need a buffer with a pH of 4.9. Which conjugate acid-base pair should you use? O sodium hydrogen carbonate (NaHCO3, pKa = 10.3) and sodium carbonate (Na2CO3) O hydrocyanic acid (HCN, pKa = 9.3) and potassium cyanide (LİCN) O hypochlorous acid (HCIO, pKa = 7.5) and potassium hypochlorite (KCIO) O acetic acid (HC2H3O2, pKa = 4.8) and sodium acetate (NaC2H3O2)

Q: What is the pH value of the final solution when 50 mL of a 0.5 M NaOH solution is added to 50 mL of…

A: Given: Volume of NaOH = 50 mL Molarity of NaOH = 0.5 M Volume of acetic acid = 50 mL Molarity of…

Q: Lemons get their sour flavor from citric acid (Ka = 7.4 x 10-4) a fresh squeezed lemon can have a…

A:

Q: Calculate the pH of a buffer system containing 3.0 M NH3 and 2.0 M NH CI. (K, of NH4, the acid in…

A: Check the formula to calculate the pH of the buffer system and use it to calculate the pH of the…

Q: Calculate the pH of a buffer solution that contains 0.34M benzoic acid and 0.49 M potassium…

A: Using Henderson equation , we can solve this problem. Here benzoic acid is weak acid and potassium…

Q: How many moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer…

A: Introduction:  We have to calculate number of moles of NaOH . Given : pH = 3.70  Ka= 6.8 × 10-4

Q: Suppose you want to make a buffer with a pH of 3.60. Which of the following acid/conjugate base…

A: The pKa value of the acid gives an idea of which conjugate acid-base pair should be chosen for the…

Q: The dissociation constant of lactic acid, a monoprotic acid found in sour milk, is 1.4 x 104. A…

A: 1) The given solution is not a buffer, as a buffer is formed by a weak acid and a salt of that weak…

Q: The bicarbonate/ carbonic acid buffer is of extreme importance to our bodies. The pH of importance…

A:

Q: A student needs to prepare a buffer solution with a pH of 5.73. Assuming a pKa of 4.06, how many mL…

A: Given,Molarity of NaOH = 0.1 MMolarity of acid ( HB ) = 0.1 Mvolume of HB = 15.0 mLpH of the buffer…

Q: Which of the following acids should be used to prepare a buffer with a pH of 3.4? CH3COОН, Ка - 1.8…

A:

Q: How many moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer…

A: Write Henderson Hasselbalch equation, pH = pKa + log[base][acid] where Ka is the acid dissociation…

Q: calculate the pH of a solution that is made when 0.10 L of 0.24 M benzoic acid (pKa=4.19) and 3.00 g…

A: Molarity of sodium benzoate can be calculated as follows:

Q: Which acid would be best to use when preparing a buffer with a pH of 4.72? A list of Ka values can…

A:

Q: Calculate the pH of a buffer comprised of 0.10 M hypochlorous acid and 0.080 M sodium hypochlorite.…

A: Formula used:-  pH = pKa + log [salt]/[acid]

Q: Calculate the pH of a buffer solution containing 0.716 mol HA weak acid and 0.607 mol A- in 239.9 mL…

A: Answer:- This question is answered by using the simple concept of calculation of pH of a buffer…

Q: How many moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer…

A: Recall the reaction that will occur here HF + NaOH→ NaF + H2OHere,we recall Henderson Hasselbalch…

Q: What concentration of sodium benzoate must be used to create a buffer solution with a pH of 5.63 if…

A: Use a udic buffer equation to get MOLARITY of sodium benzoate. Buffer mixture is defined as an…

Q: You find a solution that contains exactly 69 mM of a weak base. Adding the conjugate acid (pKa =…

A:

Q: Which of the following could you add to a solution of the weak acid, hydrosulfuric acid (H2S), to…

A: answer- hydrosulphuric acid 's conjugate base , HS- added to the solution of weak acid , H2S to make…

Q: What quantity in moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a…

A:

Q: Can someone show me how to answer this problem and the chemical equation of the buffer solution?

A: pH of a buffer solution is given by: Ka = 1.76×10-5 Substituting the values in equation (1):…

Q: How many grams of NaOH must be added to 1.50 L of a 0.400 M solution of oxoacetic acid (HCOCO2H) to…

A:

Q: What quantity in moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a…

A:

Q: What is the pH of a buffer that has 0.150 mol HC2H3O2 and 0.120 mol NaC2H3O2 in 2.00 L that has…

A:

Q: Which of the following weak acids would be suitable for making a buffer at pH = 3.50? chlorous acid…

A:

Q: Lactate is an important component in some intravenous solutions. Given pKa = 3.86 for lactic acid,…

A: pH = pKa  +  log ( [ conjugate base ]/[weak acid] ) ---------(i) pKa = 3.86 ( given) HC3H5O3…

Q: How many moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer…

A:

Q: An analytical chemist is titrating 101.8 mL of a 1.100M solution of benzoic acid (HC HCO₂) with a…

A: A solution of benzoic acid 1.100M x 101.8ml = 111.98 mmol  is titrated with 0.2600 M × 514.6 ml  =…

Q: Calculate the pH of a solution that is made when 0.10 L of  0.24 M  benzoic acid (pKa = 4.19)  and…

A: Mass of sodium benzoate = 3.00 g Molar mass of sodium benzoate = 144.11 g/mol Moles =…

Q: 3 60.0 ml of NaOH, the pH of the resulting solution is greater than 7. g 20.0 mL of NaOH, the pH of…

A: Mmol of formic acid = M × V     = 0.60 × 40 = 24 mmol After adding 60 mL of NaOH,  Mmol of NaOH =…

Q: A strong base, such as sodium hydroxide (NAOH), is added in a solution of 0.1 mol/L acetic acid…

A: Given:     Here we have to use the concept of buffer solution and apply the Handersons equation for…

Q: The pH of a bicarbonate-carbonic acid buffer is 6.18. Calculate the ratio of the concentration of…

A: The ratio of [H2CO3] to that of [HCO3-] is determined by using Henderson-Hasselbalch equation.

Q: What is the pH of a solution that results from mixing together equal volumes of a 0.120 M  solution…

A:

Q: What volume, in milliliters, of 0.240 M NaOH should be added to a 0.135 L solution of 0.030 M…

A: Here we have to determine the volume of 0.240M NaOH solution required to be added to 0.135L of…

Q: 5) You need to make 250.0 mL of a buffer with a pH of 4.10, in the chemical storage room you found…

A:

Q: Calculate the pH of a buffer solution prepared by dissolving 0.400 mol of cyanic acid (HCNO) and…

A: Given  Number of mole of HCNO Acid      = 0.400 mole  Number of mole of sodium cyanate   Salt  =…

Q: The Ka of hydrocyanic acid (HCN) is 4.0 × 10-10.  Determine the pH of a 0.300 mol/L solution of…

A: Ka = 4.0 × 10-10 Concentration of acid = 0.300M HCN ⇌ H+(aq) + CN-(aq) Let assume x is the…

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red. 

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.