A solution is made by mixing 0.400M in formic acid, HCOOH, and 1.00M in sodium formate, HCOONa? Ka-1.80x10-4. The total volume is 1.00L. What is the pH of this solution upon the addition of 0.056moles of NaOH? a. 4.234 O b. 4.059 O c. 10.744 O d. 3.431 O e. 3.256 O f. 9.766

Q: 4. Calculate the pH of a solution prepared by mixing 15.0 mL of 0.10 M NaOH and 30.0 mL of 0.10 M…

A:

Q: 6. After preparing 0.10 M sodium acetate to a volume of 50ml, what is the theoretical pH after…

A: IntroductionTo calculate the theoretical pH after adding 1.00 mL of 1.0 M NaOH to a 0.10 M sodium…

Q: 28. A student prepares 2.00 L of a solution containing 0.440 mol of sodium formate (HCOONa) and…

A: we have to calculate moles of NaOH that must be added to the buffer solution to adjust it's pH to…

Q: Calculate the pH of a solution formed by mixing 15.0 mL of 0.250 M HCIO with 15.0 mL of 0.315 M…

A: Answer :-  The pH of solution formed by mixing 15.0 ml 0.25 M HClO with 15.0 ml 0.315 M NaClO = 7.64…

Q: Explain why the pH of mixture C is the same as the pH of mixture A. Mixtures Conductvity (mA) pH A.…

A: Here we have to explain why the pH of mixture C is the same as the pH of mixture A-

Q: Calculate the pH of a 0.30M solution of sodium acetate (NaCH3COOo) given that the Ka of acetic acid…

A: Formula for calculating pH of as solution of a salt made from a weak acid and a strong base: pH = 7…

Q: Calculate the pH of the solution obtained by mixing 25.00 mL of 0.0745M HX and 25.00 mL of 0.0535M…

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Q: 1 Determine the pH of the resulting solutions when the following reagents are mixed. a. 25.00mL of…

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Q: 8. Identify each molecule as an acid or a base, then give the formula for the conjugate base or acid…

A: Given molecules,

Q: 3. After preparing 50 ml of 0.1 M HC2H3O2, what is the theoretical pH after adding 1 ml of 1M NaOH?…

A: The question is based on the concept of pH of the solution.  it is defined as a negative logarithm…

Q: A 16.3 mL solution of 0.100 mol L-1 HCl is titrated using 0.150 mol L-1 NaOH.   What is the pH of…

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Q: Acetic acid is a weak monoprotic acid with K₂ = 1.77 x 10-5. NaOH(s) was gradually added to 1.00 L…

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Q: III. A solution is made by adding 10-3 M HOCI and 10-3 M NaPr to water. Then, NaOH is added until…

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Q: . If BaCl2 completely dissolves in water, what is the ionic strength of a 0.0300 F solution of…

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Q: A solution is made by mixing 0.400M in formic acid, HCOOH, and 1.00M in sodium formate, HCOONa?…

A: Given -> Molarity of formic acid= 0.400 M Molarity of sodium formate = 1.00 M Ka = 1.80 × 10-4…

Q: Calculate the pH of a solution that contains the following analytical concentrations: a. 0.0400 M in…

A: (a) 0.0400 M NaH2PO4 ka1 = 7.11 x 10-3  ka2 = 6.32 x 10-8    (b) 0.0300 M NaH2AsO4 0.0500 M Na2HAsO4…

Q: 2. Determine the pH if I add 0.5 moles of NHẠC1 (s) to a 5 L solution of water. (Note: the Ka of…

A:

Q: S.No SOLUTION H* OH- pH РОН 1 0.15 М НI 2 0.040M KOH 3 0.020M Ва(ОН). 4 0.00030M ----- -- HCIO, 5…

A: As you not specified so i am giving first 3 answers as per guidlines Use the relation  Ph=-log(H+)…

Q: mass of NaCH3COO must be dissolved in 400 mL of 0.46 M CH3COOH in order to prepare a solution with…

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Q: 16. The Ka of Hydrocyanic acid is 4.9 X 10-10 Consider a 0.050 M solution of its salt potassium…

A: To Find: To find the pH value of the salt solution.

Q: 3. Calculate the pH of a mixture of 30.00 mL of 0.4508 M HBr and 18.00 mL of 0.1162 M Ca(OH)2.…

A: Given,Molarity of HBr = 0.4508 MVolume of HBr = 30.00 mLMolarity of Ca(OH)2 = 0.1162 MVolume of…

Q: Benzoic acid (C6H5CO₂H) is a common organic acid. Consider a solution is prepared by dissolving…

A: Given that the 1..25 L of a solution is prepared by dissolving 0.780 g of benzoic acid. initial…

Q: G and h

A: Given:

Q: HASO HNO2 K = 5.0 x 10-3 K = 4.5x 104 1. You have a solution containing 70.0 mL of 0.40 M HASO and…

A: H3AsO4  is a weak acid. The solution of weak acid and its salt is called a buffer solution. The pH…

Q: 2. How many moles of HOCI should be present together with 0.50 mole of Ca(OCI)2 in a 1.00 L solution…

A: Step 1:Step 2:Step 3:Step 4:

Q: A chemist titrates 90.0 mL of a 0.3491M aniline (C6H5NH₂) solution with 0.0636M HBr solution at 25…

A: Information of question

Q: C1. Subject:- Chemistry A solution is made by mixing 120 mL of 1.5 M disodium oxalate and 75 mL of…

A: Volume of disodium oxalate = 120 mlMolarity of disodium oxalate= 1.5 MVolume of sodium oxalate= 75…

Q: Calculate the pH of a solution formed by mixing 300.0 mL of 0.15 M NH4CI with 400.0 mL of 0.20 M…

A: Given: Concentration of NH4Cl = 0.15 M Volume of NH4Cl solution added = 300.0 mL = 0.300 L…

Q: 4. Calculate the pH of a 1L solution containing 10 mL of 2 M acetic acid and 5 g of sodium acetate…

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Q: A chemist titrates 170.0 mL of a 0.3295M ammonia (NH3) solution with 0.7467M HNO3 solution at 25 °C.…

A: pH of the given solution can be calculated at equivalence point at which only salt of weak base and…

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.