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How To Calculate The Hydroxide Ion Concentration | Chemistry
How To Calculate The Hydroxide Ion Concentration | Chemistry
How To Calculate The Hydroxide Ion Concentration | Chemistry
Biology for Non-Majors I [1]
– Define buffers and discuss the role they play in human biology. The pH of a solution is a measure of its acidity or alkalinity (base)
You might have even used some to make sure the water in an outdoor swimming pool is properly treated.. This pH test measures the amount of hydrogen ions that exists in a given solution
The overall concentration of hydrogen ions is inversely related to its pH and can be measured on the pH scale (Figure 1). Therefore, the more hydrogen ions present, the lower the pH; conversely, the fewer hydrogen ions, the higher the pH
Question Video: Calculating the Hydroxide Concentration of an Aqueous Solution given the Proton Concentration [2]
An aqueous solution at 25 degrees Celsius has an H+ concentration of two times 10 to the negative nine molar. What is the value of OH− concentration to the nearest whole number?
To solve this problem, we need to understand the relationship between these two chemical species. Molecules of water can react with each other, forming the hydronium ion and the hydroxide ion
However, hydrogen ions don’t exist by themselves in solution for very long as they react easily with water to form the hydronium ion. We’ll see this expression as an equilibrium reaction, which means we can write an equilibrium expression for it.
Free Chemistry Flashcards about Chempal-Acid/Base [3]
|a chemical dye whose color is affected by acidic and basic solutions||acid-base indicator|. |the value of the equilibrium constant expression for the ionization of a weak acid||acid ionization constant|
|describes water and other substances that can act as both acids and bases||amphoteric|. |states that an acid is a substance that contains hydrogen and ionizes to produce hydrogen ions in aqueous solutions and a base is a substance that contains a hydroxide group and dissociates to produce hydroxide ions in an aqueous solution||Arrhenius model|
|a solution that contains more hydroxide ions than hydrogen ions||basic solution|. |states an acid is a hydrogen ion donor and a base is a hydrogen ion acceptor||Bronsted-Lowery model|
What statements correctly describes the hydronium-hydroxide balance in the given solution? [4]
In neutral solutions, [H3O+] = [H2O].In bases, [OH-] = [H3O+].In bases, [OH-] is greater than [H3O+].In acids, [OH-] is greater than [H3O+].In bases, [OH-] is less than [H3O+].. Some crystals will break if they cool rapidly, some crystals will not form correctly if the solution cools too quickly.
Fehling’s solution A= concentrated aqueous solution of Copper (II) sulphate, Fehling’s solution B= solution of Sodium-potassium tarterate + sodium hydroxide.. sugar molecules are widely spreaded and are moving at random motion
Hypotonic is the term describes a solution that has a lower solute concentration and higher water concentration than another solution Hypertonic describes a solution with a higher solute concentration compared with another solution.
7.2: pH and pOH [5]
– Explain the characterization of aqueous solutions as acidic, basic, or neutral. – Use the ion-product constant for water to calculate hydronium and hydroxide ion concentrations
The concentrations of these ions in a solution are often critical determinants of the solution’s properties and the chemical behaviors of its other solutes, and specific vocabulary has been developed to describe these concentrations in relative terms. A solution is neutral if it contains equal concentrations of hydronium and hydroxide ions; acidic if it contains a greater concentration of hydronium ions than hydroxide ions; and basic if it contains a lesser concentration of hydronium ions than hydroxide ions.
One such scale that is very popular for chemical concentrations and equilibrium constants is based on the p-function, defined as shown where “X” is the quantity of interest and “log” is the base-10 logarithm:. The pH of a solution is therefore defined as shown here, where [H3O+] is the molar concentration of hydronium ion in the solution:
The pH scale [6]
The term pH is an abbreviation for power of Hydrogen, which is a measure of how acidic or basic a chemical solution is. Most solutions are either acidic or basic (also called “alkaline”) – a substance that is neither acidic nor a basic is “neutral”.[2]
One example in the context of energy is acid rain, which is formed when water interacts with various pollutants in the atmosphere. Pollutants dissolved in the rain water cause it to be acidic, which can cause damage to the environment and man-made structures
In general, a small pH value describes a solution that is acidic, and a larger pH value describing solutions that are less acidic (more basic). The pH scale is centered on 7 – meaning that a solution with a pH of 7 is perfectly neutral (neither acidic nor basic)
2.4: Acids and Bases [7]
– Define the terms pH, neutral, acidic, and basic (or alkaline). – Define the term buffer, and compare the response of a regular solution with a buffer solution to the addition of acid or base
In a strong acid, such as hydrochloric acid (HCl), all hydrogen ions (H+), and chloride ions (Cl-) dissociate (separate) when placed in water and these ions are no longer held together by ionic bonding. In a weak acid, such as carbonic acid (H2CO3), only some of the ions dissociate into hydrogen ions (H+) and bicarbonate ions (HCO3-), while others are still held together by ionic bonding.
The hydroxyl ions (OH-) released will combine with any hydrogen ions (H+) in the solution to form water molecules (OH- + H+ = H2O), so we can also define a base as a substance that takes or accepts hydrogen ions (H+) already present in the solution.. Sodium hydroxide (NaOH) is a strong base because when placed in water, it dissociates completely into sodium ions (Na+) and hydroxyl ions (OH-), all of which are now released and dissolved in water.
Concentration of Hydrogen Ions [8]
Next arises the question of what determines the acidity or alkalinity of a solution.. Actually, it is determined by the concentration of hydrogen ions, the percentage of hydrogen ions contained in the solution.
However, a very tiny percentage of those molecules have broken up into hydrogen ions (H+) and hydroxide ions, (OH-), as illustrated in the figure.. Actually, this balance of hydrogen ions and hydroxide ions determines the pH of the water.
If the reverse is true, then the solution is alkaline.. If the temperature does not vary, the following relationship between the densities of hydrogen ions (H+) and hydroxide ions (OH-) is found with any solution:
Theories of acids and bases [9]
This page describes the Arrhenius, Bronsted-Lowry, and Lewis theories of acids and bases, and explains the relationships between them. It also explains the concept of a conjugate pair – an acid and its conjugate base, or a base and its conjugate acid.
The Arrhenius theory is of historical interest only, and you are unlikely to need it unless you are doing some work on the development of ideas in chemistry.. Neutralisation happens because hydrogen ions and hydroxide ions react to produce water.
In both cases, you get a colourless solution which you can crystallise to get a white salt – either sodium chloride or ammonium chloride.. In the sodium hydroxide case, hydrogen ions from the acid are reacting with hydroxide ions from the sodium hydroxide – in line with the Arrhenius theory.
Water and neutral solutions [10]
The pH scale measures the acidity or alkalinity of a solution. Alkalis dissolve in water to give a pH greater than 7
\[H_{2}O(l)\rightleftharpoons H^{+}(aq)+OH^{-}(aq)\]. A small proportion of water molecules break up to form hydrogen ions and hydroxide ions
This is called an equilibrium and is present in water and all aqueous solutions.. In water and neutral solutions, the concentration of hydrogen ions is equal to the concentration of hydroxide ions.
16.4 Introduction to pH and pOH – Enhanced Introductory College Chemistry [11]
– Explain the characterization of aqueous solutions as acidic, basic, or neutral. – Express hydronium and hydroxide ion concentrations on the pH and pOH scales
The concentrations of these ions in a solution are often critical determinants of the solution’s properties and the chemical behaviours of its other solutes, and specific vocabulary has been developed to describe these concentrations in relative terms. A solution is if it contains equal concentrations of hydronium and hydroxide ions; if it contains a greater concentration of hydronium ions than hydroxide ions; and if it contains a lesser concentration of hydronium ions than hydroxide ions
For a brief introduction into the pH scale and how it is used, Watch The pH Scale Explained (5min 54s).. The is a scale of acidity ranging 0 to 14 (but not always)
8.3 pH and pOH – Inorganic Chemistry for Chemical Engineers [12]
– Explain the characterization of aqueous solutions as acidic, basic, or neutral. – Express hydronium and hydroxide ion concentrations on the pH and pOH scales
The concentrations of these ions in a solution are often critical determinants of the solution’s properties and the chemical behaviors of its other solutes, and specific vocabulary has been developed to describe these concentrations in relative terms. A solution is neutral if it contains equal concentrations of hydronium and hydroxide ions; acidic if it contains a greater concentration of hydronium ions than hydroxide ions; and basic if it contains a lesser concentration of hydronium ions than hydroxide ions.
One such scale that is very popular for chemical concentrations and equilibrium constants is based on the p-function, defined as shown where “X” is the quantity of interest and “log” is the base-10 logarithm:. The pH of a solution is therefore defined as shown here, where [H3O+] is the molar concentration of hydronium ion in the solution:
Wikipedia [13]
In chemistry, pH (/piːˈeɪtʃ/ pee-AYCH), also referred to as acidity, historically denotes “potential of hydrogen” (or “power of hydrogen”).[1] It is a scale used to specify the acidity or basicity of an aqueous solution. Acidic solutions (solutions with higher concentrations of hydrogen (H+) ions) are measured to have lower pH values than basic or alkaline solutions.
where [H+] is the equilibrium molar concentration (mol/L) of H+ in the solution. At 25 °C (77°F), solutions with a pH less than 7 are acidic, and solutions with a pH greater than 7 are basic
The neutral value of the pH depends on the temperature and is lower than 7 if the temperature increases above 25 °C. The pH range is commonly given as zero to 14, but a pH value can be less than 0 for very concentrated strong acids or greater than 14 for very concentrated strong bases.[3]
Regents Chemistry Exam Multiple Choice Practice Questions And Solutions: Acids And Bases Topic [14]
Solution: According to the Bronsted Lowry acid-base theory, acid is a proton (H+) donor and base is a proton acceptor.. 27 The acidity or alkalinity of a solution can be measured by its (1) pH value (2) electronegativity value
pH of 0-7 is acidic, 7 is neutral and 7-14 is basic.. 26 As more NaCl(s) is dissolved in a dilute, unsaturated NaCl(aq) solution, the conductivity of the solution (1) decreases as the ion concentration decreases
NaCl is an ionic compound that dissociates into ions, which makes the solution capable of conducting electricity. As more NaCl is added, more ions are produced which in turn increases the conductivity of the solution.
How to Calculate pH: Explanation, Review, and Examples [15]
pH is a unit of measurement often used in fundamental chemistry concepts. “How to Calculate pH” explains its categories, scientific mathematics, and the role pH has in our lives.
This unit was introduced by biochemist Søren Peter Lauritz Sørensen in 1909. It was an easy way to represent the concentration of hydrogen ions in a solution during titrations
For acids, one of those ions is a hydrogen ion (H+) and for bases, one of the ions is a hydroxide ion (OH–). This description of acids and bases is known as the Arrhenius Theory
Acids and Bases [16]
Acids and bases are popular chemicals which interact with each other resulting in the formation of salt and water. The word acid comes from a Latin word ‘acere’ which means ‘sour’.
The orange or grapefruit juice you drink for breakfast contains citric acid (also known as Vitamin C). The vinegar used in salad dressing contains acetic acid
The properties of a molecule, therefore, can be understood by dividing it into acid and base fragments.. An acid is any hydrogen-containing substance that is capable of donating a proton (hydrogen ion) to another substance
Acids and bases: 8.11 [17]
Arrhenius acids are substances that provide free hydrogen ions in aqueous solution.. Arrhenius’ definition of an acid is the one that most people are familiar with, a substance that produces hydrogen ions in water:
This is because all acids contain these free H+ ions (hydrogen ions) in solution. The hydrogen ion is effectively a single proton, whose charge density (charge/volume ratio) is very large
Although the hydrogen ions are bonded to the water molecules, this does not really make much difference, as we can simply deal with acids as solutions containing free hydrogen ions.. 1 Acids turn indicators characteristic colours (the actual colour depends on the indicator).
A solution that contains equal numbers of hydrogen and hydroxide ions is: a. Alkaline b. Acidic c. Basic d. Neutral [18]
A solution that contains equal numbers of hydrogen and hydroxide ions is: a. A solution that contains equal numbers of hydrogen and hydroxide ions is:
An acidic substance falls in the pH range of 1-6, and a basic substance falls in the range of 8-14. Become a Study.com member to unlock this answer! Create your accountView this answer
An acidic substance has more hydrogen ions than hydroxide. Our experts can answer your tough homework and study questions.Ask a question Ask a question
The pH Scale [19]
Whether a liquid is an acid or a base has to do with hydrogen ions (abbreviated with the chemical symbol H+). In water (H2O), a small number of the molecules dissociate (split up)
The “lost” hydrogen ions join up with water molecules to form hydronium ions (H3O+). For simplicity, hydronium ions are referred to as hydrogen ions H+
Because of this, when an acid is dissolved in water, the balance between hydrogen ions and hydroxide ions is shifted. Now there are more hydrogen ions than hydroxide ions in the solution
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